Match the following aqueous solutions with the appropriate letter from the column on the right. Assume complete dissociation of electrolytes. D 1. 0.11 m Fe(NO3)3 A. Lowest freezing point C 2. 0.18 m NaOH B. Second lowest freezing point B 3. 0.21 m FeSO4 C. Third lowest freezing point A 4. 0.38 m Glucose (nonelectrolyte) D. Highest freezing point An error has been detected in your answer. Check

Answer:

233 g

Explanation:

Let's consider the following reaction.

CaCO₃ → CaO + CO₂

We can establish the following relations:

The mass of carbon dioxide produced from 530 g of calcium carbonate is:

[tex]530gCaCO_{3}\frac{1molCaCO_{3}}{100.09gCaCO_{3}} ,\frac{1molCO_{2}}{1molCaCO_{3}} .\frac{44.01gCO_{2}}{1molCO_{2}} =233gCO_{2}[/tex]

233 gram of carbon dioxide gas is produced from the decomposition of calcium carbonate.

[tex]CaCO_3\rightarrow CaO + CO_2[/tex]

From the above decomposition, we can say that the molar ratio of calcium carbonate to carbon dioxide is 1:1.

The molar mass of calcium carbonate is 100.09 g/mol.

The molar ratio of calcium carbonate to carbon dioxide is 1:1.

The molar mass of carbon dioxide is 44.01 g/mol

The mass of carbon dioxide produced from 530 g of calcium carbonate is:

[tex]{530\ gCaCO_3}\times\frac{1molCaCO_3}{100gCaCO_3} \times\frac{1molCO_2}{1molCaCO_3} \times\frac{44.01\ gCO_2}{1molCO_2} =233\ gCO_2[/tex]

So, the 233 g [tex]CO_2[/tex] will be produced.

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Answer:

0.218 M of Pb(NO3)2

Explanation:

Equation of the reaction

Pb(NO3)2(aq) + 2NaCl(aq) --> PbCl2(s) + 2NaNO3(aq)

1 mole of Pb(NO3)2 reacts to precipitate 1 mole of PbCl2

Molar mass of PbCl2 = 207 + (35.5*2)

= 278 g/mol

Number of moles of PbCl2 precipitated = mass/molar mass

= 12.11/278

= 0.04356 mol

Since 0.04356 moles of PbCl2 was precipitated, therefore by stoichiometry; 0.04356 moles of Pb(NO3)2 reacted.

Molarity is defined as the number of moles of solute in 1 liter of solution.

Molarity = number of moles/volumes

= 0.04356/0.2

= 0.218 M

Compound A is an optically active ketone, B is a chiral secondary alcohol, and C is an alkene formed from A by a Wolff-Kishner reduction. Acid D is a carboxylic acid crafted from the oxidation of alkene C.

This problem involves the identification of chemical compounds through a series of reactions and stereochemical considerations. We start by identifying compound A as an optically active ketone with the molecular formula C11H12O, since it gave a negative Tollens test. LiAlH4, a strong reducing agent, follows by acid treatment, produces compound B, an alcohol that can be resolved into enantiomers, suggesting that compound A must be a ketone, as LiAlH4 can reduce ketones to secondary alcohols, which can be chiral.

When compound B reacts with CrO3/pyridine, it reverts to the optically inactive ketone compound A. This suggests that compound B is a secondary alcohol that, when oxidized, returns to the original ketone without any chirality, indicating the presence of a stereocenter in B.

Heating compound A with hydrazine in base to give hydrocarbon C suggests a Wolff-Kishner reduction, which completely removes oxygen atoms from ketones or aldehydes to yield hydrocarbons. Finally, when compound C is oxidized with alkaline KMnO4 to give carboxylic acid D, this indicates that C is an alkene.

Compound A is Ketone, Compound B is chiral alcohol, Compound C is hydrocarbon, Compound D is carboxylic acid.

Let's break down the given information step by step:

1. Compound A, [tex]C_{11}H_{12}O[/tex], gave a negative Tollens test:

This suggests that compound A does not contain an aldehyde functional group. Instead, it may contain a ketone or another functional group that does not react with Tollens reagent.

2. Compound A was treated with [tex]LiAlH_4[/tex], followed by dilute acid, to give compound B, which could be resolved into enantiomers:

The reduction of a ketone with [tex]LiAlH_4[/tex] followed by hydrolysis with dilute acid converts the ketone to a chiral alcohol. Since compound B can be resolved into enantiomers, it suggests that compound A was a prochiral ketone.

3. When optically active B was treated with [tex]CrO_3[/tex] in pyridine, an optically inactive sample of A was obtained:

This reaction is a oxidation reaction known as the Jones oxidation. It converts a secondary alcohol (like B) into a ketone without affecting the optical activity. However, since an optically inactive sample of A was obtained, it suggests that compound B must have been racemic (an equal mixture of its enantiomers). This indicates that the chiral center in compound B was destroyed during the oxidation.

4. Heating A with hydrazine in base gave hydrocarbon C, which, when heated with alkaline KMnO4, gave carboxylic acid D:

Heating a ketone with hydrazine in base (Wolff-Kishner reduction) converts it into a hydrocarbon. This indicates that compound A was a ketone. Furthermore, oxidation of hydrocarbon C with alkaline [tex]KMnO_4[/tex]gives a carboxylic acid. This suggests that hydrocarbon C must have been a primary alcohol.

The alkali metal cation in the unknown metal hydroxide that has been reacted with hydrochloric acid is Potassium (K+). The identity of the cation was determined by performing a stoichiometric calculation based on the balanced chemical reaction and the molar masses of the alkali metal hydroxide.

This is a stoichiometry problem that requires understanding of acid-base titration reactions. In a neutralization reaction, an acid reacts with a base to form water plus a salt. Here, the hydrochloric acid (HCl) is reacting with the alkali metal hydroxide (MOH) to form water (H2O) and a salt (MCl). The balanced chemical reaction is HCl + MOH -> H2O + MCl.

The mole ratio between HCl and MOH in this reaction is 1:1. This means that for each mole of HCl used, one mole of MOH will react. From the volume (17.0 mL) and molarity (2.5 M) of HCl used, we can calculate the number of moles of HCl, which will also be the number of moles of MOH because of the 1:1 mole ratio.

mol HCl = Molarity x Volume = 2.50 mol/L x 17.0 x 10-3 L = 0.0425 mol. Hence, the number of moles of MOH = 0.0425 mol.

The molar mass of alkali metal hydroxide (MOH) is its mass divided by the number of moles. Hence, Molar mass = mass (g) / moles = 4.36 g / 0.0425 mol = 102.59 g/mol. This molar mass is closest to the molar mass of Potassium Hydroxide (KOH), which is 39.10 (K) + 15.9994 (O) + 1.00784 (H) = 56.11 g/mol. So, the alkali metal cation in the unknown metal hydroxide is K+ (Potassium).

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The provided unknown sample contains Rubidium (Rb⁺) as its alkali metal cation. This conclusion is based on titration calculations, yielding a molar mass closest to Rb.

To identify the alkali metal cation (Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺) from the given sample, we need to perform a titration calculation. Here are the steps:

First, calculate the moles of HCl used in the titration:

The balanced equation for the reaction is:

MOH + HCl → MCl + H2O

Since the reaction is 1:1, moles of MOH = moles of HCl = 0.0425 mol

Next, calculate the molar mass of the alkali metal hydroxide (MOH):

Given MOH is an alkali metal hydroxide, its molar mass is the sum of the molar masses of M, O, and H, which is represented as:

M + 17.01 (since the molar mass of OH is 17.01 g/mol)

Therefore, M = 102.59 - 17.01 ≈ 85.58 g/mol

Match this result with the molar masses of the alkali metals:

The metal with a molar mass closest to 85.58 g/mol is Rb (Rubidium).

Therefore, the alkali metal cation is Rb⁺ (Rubidium).

Answer and Explanation

The isomer picked is the N-Propylamine.

It has a lone pair of electron available on the electron rich Nitrogen and no formal charge.

Since it will be hard to draw the Lewis structure in this answer format, I'll attach a picture of the Lewis structure to this answer.

The lone pair of electron is shown by the two dots on the Nitrogen atom.

The Lewis structure for propylamine is drawn by connecting a chain of three carbon atoms with the appropriate number of hydrogen atoms, and attaching the nitrogen atom to the third carbon with two of its own hydrogen atoms and a lone pair, ensuring all atoms follow the octet rule without any formal charges.

To draw the Lewis structure for propylamine (CH₃(CH₂)₂NH₂), you should follow the basic rules of drawing Lewis structures and consider the number of valence electrons that each atom has. Carbon (C) has 4 valence electrons, Hydrogen (H) has 1, and Nitrogen (N) has 5. Here's the step-by-step breakdown:

In propylamine, no formal charges are present as all the atoms have the correct number of electrons around them for neutrality. The nitrogen atom has a free lone pair and there are no pi bonds, so each bond is a single bond.

Answer:

(a) 6g. Shell 6, n = 6. Subshell g, l = 4. Number of orbitals in sublevel = 9

(b) 4s. Shell 4, n = 4. Subshell s, l = 0. Number of orbitals in sublevel = 1

(c) 3d. Shell 3, n = 3. Subshell d, l = 2. Number of orbitals in sublevel = 5

Explanation:

The rules for electron quantum numbers are:

1. Shell number, 1 ≤ n, n = 1, 2, 3...

2. Subshell number, 0 ≤ l ≤ n − 1, orbital s - 0, p - 1, d - 2, f - 3

3. Orbital energy shift, -l ≤ ml ≤ l

4. Spin, either -1/2 or +1/2

So,

(a) 6g. Shell 6, n = 6. Subshell g, l = 4. Number of orbitals in sublevel = 2l+1 = 9

(b) 4s. Shell 4, n = 4. Subshell s, l = 0. Number of orbitals in sublevel = 2l+1 = 1

(c) 3d. Shell 3, n = 3. Subshell d, l = 2. Number of orbitals in sublevel = 2l+1 = 5

(a) 6g Shell 6, n = 6. Subshell g, l = 4. Number of orbitals in sublevel = 9

(b) 4s Shell 4, n = 4. Subshell s, l = 0. Number of orbitals in sublevel = 1

(c) 3d Shell 3, n = 3. Subshell d, l = 2. Number of orbitals in sublevel = 5

There are a total of four quantum numbers: the principal quantum number (n), the orbital angular momentum quantum number (l), the magnetic quantum number (ml), and the electron spin quantum number (ms).

The rules for electron quantum numbers are:

1. Shell number, 1 ≤ n, n = 1, 2, 3...

2. Subshell number, 0 ≤ l ≤ n − 1, orbital s - 0, p - 1, d - 2, f - 3

3. Orbital energy shift, -l ≤ ml ≤ l

4. Spin, either -1/2 or +1/2

(a) 6g. Shell 6, n = 6. Subshell g, l = 4. Number of orbitals in sublevel = 2l+1 = 9

(b) 4s. Shell 4, n = 4. Subshell s, l = 0. Number of orbitals in sublevel = 2l+1 = 1

(c) 3d. Shell 3, n = 3. Subshell d, l = 2. Number of orbitals in sublevel = 2l+1 = 5

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Answer:

The answers indicate that wavelength is inversely proportional to the energy of light (photon)

Explanation:

Energy of photon E = hc/λ

where;

h is Planck's constant = 6.626 X 10⁻³⁴js

c is the speed of light (photon) = 3 X 10⁸ m/s

λ is the wavelength of the photon

⇒For ultraviolet ray, with wavelength λ = 1 x 10⁻⁸ m

E = (6.626 X 10⁻³⁴ X 3 X 10⁸)/ (1 x 10⁻⁸)

E = 19.878 10⁻¹⁸ J

⇒For Visible light, with wavelength λ = 5 x 10⁻⁷ m

E = (6.626 X 10⁻³⁴ X 3 X 10⁸)/ (5 x 10⁻⁷)

E = 3.9756 X 10⁻¹⁹ J

⇒For Infrared, with wavelength λ = 1 x 10⁴ m

E = (6.626 X 10⁻³⁴ X 3 X 10⁸)/ (1 x 10⁴)

E = 19.878 X 10⁻³⁰ J

From the result above, ultraviolet ray has the shortest wavelength, but it has the highest energy among other lights.

Also infrared has the highest wavelength but the least energy among other lights.

Hence, wavelength is inversely proportional to the energy of light (photon).

The energies of one photon of ultraviolet (λ = 1 x 10⁻⁸ m), visible (λ = 5 x 10⁻⁷ m), and infrared (λ = 1 x 10⁴ m) light are [tex]1.988 \times 10^{-17} \, \text{J} \),[/tex]  [tex]3.98 \times 10^{-19} \, \text{J} \),[/tex] [tex]1.99 \times 10^{-30} \, \text{J} \)[/tex] respectively. The answers indicate that as the wavelength of light decreases, the energy of the photons increases.

To calculate the energy of a photon, we use the formula:

[tex]\[ E = \frac{hc}{\lambda} \][/tex]

where:

- E is the energy of the photon

- h  is Planck's constant [tex](\( 6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \))[/tex]

- c is the speed of light in a vacuum [tex](\( 3.00 \times 10^8 \, \text{m/s} \))[/tex]

- [tex]\( \lambda \)[/tex] is the wavelength of the photon

Let's calculate the energy for each type of light:

Ultraviolet Light (λ = 1 x 10⁻⁸ m)

[tex]\[ E_\text{UV} = \frac{6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \times 3.00 \times 10^8 \, \text{m/s}}{1 \times 10^{-8} \, \text{m}} \][/tex]

Visible Light (λ = 5 x 10⁻⁷ m)

[tex]\[ E_\text{Visible} = \frac{6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \times 3.00 \times 10^8 \, \text{m/s}}{5 \times 10^{-7} \, \text{m}} \][/tex]

Infrared Light (λ = 1 x 10⁴ m)

[tex]\[ E_\text{IR} = \frac{6.626 \times 10^{-34} \, \text{J} \cdot \text{s} \times 3.00 \times 10^8 \, \text{m/s}}{1 \times 10^4 \, \text{m}} \][/tex]

Let's compute these values:

1. Ultraviolet Light:

[tex]\[ E_\text{UV} = \frac{6.626 \times 10^{-34} \times 3.00 \times 10^8}{1 \times 10^{-8}} \][/tex]

[tex]\[ E_\text{UV} = \frac{19.878 \times 10^{-26}}{1 \times 10^{-8}} \][/tex]

[tex]\[ E_\text{UV} = 19.878 \times 10^{-18} \][/tex]

[tex]\[ E_\text{UV} = 1.988 \times 10^{-17} \, \text{J} \][/tex]

2. Visible Light:

[tex]\[ E_\text{Visible} = \frac{6.626 \times 10^{-34} \times 3.00 \times 10^8}{5 \times 10^{-7}} \]\[ E_\text{Visible} = \frac{19.878 \times 10^{-26}}{5 \times 10^{-7}} \]\[ E_\text{Visible} = 3.9756 \times 10^{-19} \]\[ E_\text{Visible} = 3.98 \times 10^{-19} \, \text{J} \][/tex]

3. Infrared Light:

[tex]\[ E_\text{IR} = \frac{6.626 \times 10^{-34} \times 3.00 \times 10^8}{1 \times 10^4} \]\[ E_\text{IR} = \frac{19.878 \times 10^{-26}}{1 \times 10^4} \]\[ E_\text{IR} = 1.9878 \times 10^{-30} \]\[ E_\text{IR} = 1.99 \times 10^{-30} \, \text{J} \][/tex]

Summary of Energies

- Ultraviolet Light (λ = 1 x 10⁻⁸ m): [tex]\( E_\text{UV} = 1.988 \times 10^{-17} \, \text{J} \)[/tex]

- Visible Light (λ = 5 x 10⁻⁷ m): [tex]\( E_\text{Visible} = 3.98 \times 10^{-19} \, \text{J} \)[/tex]

- Infrared Light (λ = 1 x 10⁴ m): [tex]\( E_\text{IR} = 1.99 \times 10^{-30} \, \text{J} \)[/tex]

Relationship between Wavelength and Energy

Specifically:

- Ultraviolet light has the shortest wavelength and the highest energy.

- Visible light has a moderate wavelength and moderate energy.

- Infrared light has the longest wavelength and the lowest energy.

This inverse relationship between wavelength and photon energy is consistent with the equation [tex]\( E = \frac{hc}{\lambda} \)[/tex]. As [tex]\( \lambda \) (wavelength) decreases, \( E \)[/tex] (energy) increases, and vice versa.

Answer:

The rate of the reaction increased by a factor of 1012.32

Explanation:

Applying Arrhenius equation

ln(k₂/k₁) = Ea/R(1/T₁ - 1/T₂)

where;

k₂/k₁ is the ratio of the rates which is the factor

Ea is the activation energy = 274 kJ/mol.

T₁ is the initial temperature = 231⁰C = 504 k

T₂ is the final temperature = 293⁰C = 566 k

R is gas constant = 8.314 J/Kmol

Substituting this values into the equation above;

ln(k₂/k₁) = 274000/8.314(1/504 - 1/566)

ln(k₂/k₁) = 32956.4589 (0.00198-0.00177)

ln(k₂/k₁)  = 6.92

k₂/k₁ = exp(6.92)

k₂/k₁ = 1012.32

The rate of the reaction increased by 1012.32

Answer:

By a factor of 2.25.

Explanation:

Using the Arrhenius equations for the given conditions:

k1 = A*(exp^(-Ea/(RT1))

k2 = A*(exp^(-Ea/(RT2))

T1 = 231°C

= 231 + 273.15 K

= 574.15 K

T2 = 293°C

= 293 + 273.15 K

= 566.15 K

Ea = 274 kJ mol^-1

R= 0.008314 kJ/mol.K

Now divide the second by the first:

k2/k1 = exp^(-Ea/R * (1/T2 - (1/T1))

= 0.444

2.25k2 = k1

Answer:

At least 3 three extractions are required to recover at least 99.5 % of the material in the organic layer.

Explanation:

The partition coefficient of a solute (S) soluble in two immiscible solvents is given by the following formula

[tex]K_S=\frac{[S]_2}{[S]_1}[/tex]

The lower layer is taken as an aqueous layer (1), while the upper layer is organic (2). The fraction of solute remaining in the aqueous layer is given by the following formula

[tex]q^n=(\frac{V_1}{V_1 \times KV_2})^n[/tex]

Here, n denotes the number of extraction, and q^n represents the fraction of solute remaining in aqueous solvent after n number of extraction. According to the given data, the fraction of solute remaining in the aqueous layer after multiple extractions is 0.005, i.e., q^n=0.005. Mathematically,

[tex]0.005=(\frac{50}{50 + 50\times10})^n\\\\0.005=(0.091)^n[/tex]

Taking log on both sides

[tex]log(0.005)=nlog(0.091)[/tex]

[tex]log(0.005)=nlog(0.091)\\\\-2.301=-n1.04\\n=2.21[/tex]

The above calculations show that the number of extractions should be greater than 2, i.e, at least 3, in order to achieve extraction greater than 99.5 %.

With a partition coefficient of 10 and using 50mL each of water and ether, approximately three extractions are required to recover at least 99.5% of the material in the organic layer.

This question relates to an extraction process used in chemistry. The extraction process is governed by a partition coefficient, which is the ratio of the concentrations of a compound in the two solvents (organic layer and water in this case) at equilibrium. To calculate the number of extractions required to recover at least 99.5% of the material, we can use the formula:

Where D is the partition coefficient. By rearranging this equation, we get:

Substituting the given values into the equation, we find that approximately 3 extractions would be required in order to recover at least 99.5% of the material in the organic layer.

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The rate changes by a factor of 1/16 when the concentration of H+ is decreased by a factor of 4 in the given rate law.

The reaction with the rate law Rate = k{BrO3-}{Br-}{H+}2 indicates that the rate of the reaction is directly proportional to the concentration of H+ raised to the second power. Thus, if the concentration of H+ is decreased by a factor of 4, the rate of the reaction would decrease by a factor of 42 or 16. Therefore, the rate changes by a factor of 1/16 when the concentration of H+ decreases by a factor of 4.

The rate law for the given reaction is Rate = k{BrO3-}{Br-}{H+}^2. If the concentration of H+ is decreased by a factor of 4, it means the new concentration of H+ would be 1/4 of the original concentration. Since the rate law is quadratic with respect to H+, the rate would change by a factor of (1/4)^2, which is 1/16. Therefore, the rate would decrease by a factor of 1/16 or 0.0625.

The rate of the reaction changes by a factor of [tex]\(\frac{1}{16}\)[/tex] (or decreases to [tex]\(\frac{1}{16}\)[/tex] of its original rate) when the concentration of[tex]\( \text{H}^+ \)[/tex] is decreased by a factor of 4.

Given the reaction with the rate law:

[tex]\[ \text{Rate} = k[\text{BrO}_3^-][\text{Br}^-][\text{H}^+]^2 \][/tex]

We need to determine how the rate changes if the concentration of[tex]\( \text{H}^+ \)[/tex] is decreased by a factor of 4.

Step-by-Step Explanation:

1. Initial Rate Law Expression:

[tex]\[ \text{Rate}_1 = k[\text{BrO}_3^-][\text{Br}^-][\text{H}^+]^2 \][/tex]

2. Change in [tex]\( \text{H}^+ \)[/tex] Concentration:

  Let's denote the initial concentration of[tex]\( \text{H}^+ \)[/tex]as [tex]\([ \text{H}^+ ]_1\)[/tex]. If the concentration of[tex]\( \text{H}^+ \)[/tex] is decreased by a factor of 4, the new concentration will be:

[tex]\[ [ \text{H}^+ ]_2 = \frac{[ \text{H}^+ ]_1}{4} \][/tex]

3. New Rate Law Expression:

  Substitute the new concentration of [tex]\( \text{H}^+ \)[/tex] into the rate law:

[tex]\[ \text{Rate}_2 = k[\text{BrO}_3^-][\text{Br}^-]\left( \frac{[ \text{H}^+ ]_1}{4} \right)^2 \][/tex]

4. Simplify the Expression:

[tex]\[ \text{Rate}_2 = k[\text{BrO}_3^-][\text{Br}^-]\left( \frac{[ \text{H}^+ ]_1^2}{4^2} \right) \][/tex]

[tex]\[ \text{Rate}_2 = k[\text{BrO}_3^-][\text{Br}^-]\left( \frac{[ \text{H}^+ ]_1^2}{16} \right) \][/tex]

5. Relate [tex]\( \text{Rate}_2 \) to \( \text{Rate}_1 \)[/tex] :

  From the initial rate law, we know that:

 [tex]\[ \text{Rate}_1 = k[\text{BrO}_3^-][\text{Br}^-][\text{H}^+]_1^2 \][/tex]

  So, we can write:

[tex]\[ \text{Rate}_2 = \frac{\text{Rate}_1}{16} \][/tex]

6. Factor by Which the Rate Changes:

  The rate decreases by a factor of 16.

Answer:

volume of gas = 9.1436cm³

Explanation:

We will only temperature from °C to K since the conversion is done by the addition of 273 to the Celsius value.

Its not necessary to convert pressure and volume as their conversions are done by multiplication and upon division using the combined gas equation, the factors used in their conversions will cancel out.

V1 =10.1cm³ , P1 =746mmHg,     T1=23°C =23+273=296k

V2 =? ,   P2 =760mmmHg ,     T2=0°C = 0+273 =273K

Using the combined gas equation to calculate for V2;

[tex]\frac{V1P1}{T1}=\frac{V2P2}{T2} \\ re-arranging, \\V2 =\frac{V1P1T2}{P2T1}[/tex]

[tex]V2 =\frac{10.1*746*273}{760*296}[/tex]

V2=9.1436cm³

Answer:

43.47 g

Explanation:

The boiling point elevation is described as:

Where ΔT is the difference in boiling points: 120.6-118.4 = 2.2 °C

K is the boiling point elevation constant, K= 2.40 °C·kg·mol⁻¹

and m is the molality of the solution (molality = mol solute/kg solvent).

So first we calculate the molality of the solution:

Now we calculate the moles of benzamide (C₇H₇NO, MW=315g/mol), using the given mass of the liquid X.

Finally we convert moles of C₇H₇NO into grams, using its molecular weight:

Final answer:

To calculate the mass of C7H7NO dissolved in the solution, use the formula for boiling point elevation in a solution.

Explanation:

The mass of C7H7NO that was dissolved in the solution can be calculated using the formula:

ΔTb = i * K * m

Where ΔTb is the boiling point elevation, i is the van't Hoff factor (number of particles the solute dissociates into), K is the boiling point elevation constant, and m is the molality of the solution.

Substitute the given values into the equation to find the mass of C7H7NO dissolved.

Answer : The  mass of [tex]KC_2H_5CO_2[/tex] is, 24.5 grams

Explanation : Given,

[tex]K_a=1.3\times 10^{-5}[/tex]

pH = 5.02

Concentration of [tex]HC_2H_5CO_2[/tex] = 1.30 M

Volume of solution = 125 mL = 0.125 L

First we have to calculate the value of [tex]pK_a[/tex].

The expression used for the calculation of [tex]pK_a[/tex] is,

[tex]pK_a=-\log (K_a)[/tex]

Now put the value of [tex]K_a[/tex] in this expression, we get:

[tex]pK_a=-\log (1.3\times 10^{-5})[/tex]

[tex]pK_a=5-\log (1.3)[/tex]

[tex]pK_a=4.89[/tex]

Now we have to calculate the concentration of [tex]KC_2H_5CO_2[/tex]

Using Henderson Hesselbach equation :

[tex]pH=pK_a+\log \frac{[Salt]}{[Acid]}[/tex]

[tex]pH=pK_a+\log \frac{[KC_2H_5CO_2]}{[HC_2H_5CO_2]}[/tex]

Now put all the given values in this expression, we get:

[tex]5.02=4.89+\log (\frac{[KC_2H_5CO_2]}{1.30})[/tex]

[tex][KC_2H_5CO_2]=1.75M[/tex]

Now we have to calculate the moles of [tex]KC_2H_5CO_2[/tex]

[tex]\text{Moles of }KC_2H_5CO_2=1.75M\times 0.125L=0.219mol[/tex]

Now we have to calculate the mass of [tex]KC_2H_5CO_2[/tex]

[tex]\text{Mass of }KC_2H_5CO_2=\text{Moles of }KC_2H_5CO_2\times \text{Molar mass of }KC_2H_5CO_2[/tex]

Molar mass of [tex]KC_2H_5CO_2[/tex] = 112 g/mol

[tex]\text{Mass of }KC_2H_5CO_2=0.219mol\times 112g/mol=24.5g[/tex]

Thus, the mass of [tex]KC_2H_5CO_2[/tex] is, 24.5 grams

To find the mass of KC₂H₃CO₂ needed to create a buffer at pH 5.02, the Henderson-Hasselbalch equation is used to calculate the ratio of conjugate base to acid, then the molar mass is used to convert moles to mass, the concentration of A⁻ is approximately 1.755 M.

The question asks for the mass of potassium propanoate (KC₂H₃CO₂) needed to create a buffer with a specific pH from a solution of propanoic acid (KC₂H₃CO₂). To solve this, we apply the Henderson-Hasselbalch equation:

[tex]\[ pH = pKa + \log \left( \frac{[A^-]}{[HA]} \right) \][/tex]

Given variables:

Rearranging the equation to solve for A⁻:

A⁻ = [tex][HA] \times 10^{(pH - pKa)}[/tex]

A⁻ = 1.755M

After calculating A⁻, it's then converted from molarity to moles given the volume of the solution. Finally, the mass of KC₂H₃CO₂ is 1.755M by multiplying the number of moles of A⁻ by its molar mass.

Explanation:

Magnesium oxide

Answer:

Explanation:

Niobium has an anomalous ground-state electron configuration for a Group 5 element: [Kr] 5s¹4d⁴ . IT is anomalous because in normal course , it should have been [Kr] 5s²4d³ Or [Kr] 5s⁰4d⁵ . It is so because 5s subshell

has lesser energy than 4d subshell ,  or half filled 4d subshell is more stable. But the stable configuration is [Kr] 5s¹4d⁴ . It is so because the energy gap between 5s and 4d is very little. So one electron of 5s² gets Transferred to 4d subshell.  This paramagnetic behavior is confirmed by its dipole moment , equivalent to 5 unpaired electrons.

Answer:

The reaction of hex-3-yne with one equivalent of HCl Is an Anti addition, see in the drawing the major product.

Explanation:

The mechanism of the reaction proceeds through a carbocation, formed in the most substituted carbon of the triple bond,  in this case it is indistinct because the triple bond is in the central carbons. Therefore, it is a regioselective reaction that follows Markovnikov's rule, adding the halogen to the more substituted carbon of the alkyne.

The anti addition consists in the addition of two substituents on opposite sides of a triple bond, which gives it greater stability.

Answer:

Molality for the solution is 2.22 m

Explanation:

Molality is a sort of concentration. Indicated the moles of solute in 1kg of solvent. → mol/kg

Let's determine the moles of solute (mass / molar mass)

17.85 g / 92 g/mol = 0.194 moles

Let's convert the mass of solvent (g) to kg

87.4 g . 1kg / 1000 g = 0.0874 kg

Mol/kg → Molality

0.194 mol / 0.0874 kg = 2.22 m

Answer:

The answer the question, what is the pressure of the gas, in pascals is 101195.73 Pa

Explanation:

Firstly we list out the known variables

The known variables are

mass of piston = 1.1 kg, diameter of piston, D = 10.0 cm = 0.1 m

mass of weight = 2.0 kg atmospheric pressure = 1.0 atm

In this question the quantity required is the presssure of the gas in the cylinder after placing a weght on the piston

To solve this, we note that Pressure = Force per unit area

= Force/area, hence

We compute the area of the piston thus

Area = (πD²)÷4 = 0.0079 m²

While the sum of the mass of the piston and the added weight = 1.1 kg + 2.0 kg = 3.1 kg

The weight of the added mass and piston that is their force on the gas = W = Mass × gravity = 3.1 kg × 9.81 m/s² = 30.411 N

Therefore the pressure  = 30.411N/(0.0079 m²) = 3870.73 Pascals

The pressure of the gas = pressure due to the piston and the added weight + pressure due to the atmosphere

thus pressure of the gas = 3870.73 Pa + 1.0 atm =3870.73 Pa + 101325 Pa =101195.73 Pa

The pressure of the gas, in pascals is 101195.73 Pa

Answer:

195.52 g/mol

Explanation:

Answer:

195.52 g/mol

Explanation:

1.) ΔT = Kb * molality

2.) (100.22-100) = 0.512 * molality

3.) 0.22 = 0.512 * molality

4.) 0.22/0.512 =( 0.512 * molality)/ 0.512

5.) 0.4297 = molality

6.) molality = mol of solute/ kg of solvent

7.) 0.4297 = mol of solute / (0.750- 0.058125)

8.) 0.4297 = mol of solute / 0.69175

9.) (0.4297 = mol of solute / 0.69175) * 0.69175

10.) mol of solute = 0.29729

11.) mol = mass / mw therefore mw = mass/ mol

12.) mw = 58.125g / 0.29729mol

13.) mw = 195.125 g/mol

Please be mindful I did not consistently write conversions or write out units to show cancellations.

To determine the molecular weight of the unknown compound, one would need to calculate the boiling point elevation, then the molality of the solution, and finally rearrange the formula to solve for the molar mass based on the given masses of solute and solvent.

The student's question pertains to the calculation of the molecular weight of an unknown compound using the boiling point elevation method in Chemistry. To find the molecular weight of the unknown compound, the boiling point elevation (ΔTb) first needs to be determined, using the observed boiling point and the normal boiling point of water (100°C). Then, using the boiling point elevation constant (Kb for water), and the mass of the solute and solvent, the molality (m) of the solution can be calculated. The molar mass (M) of the unknown compound is then found by rearranging the formula ΔTb = i ⋅ Kb ⋅ m, where i is the van't Hoff factor (which is 1 for a nonelectrolyte compound) and solving for M.

Since we know the mass of the solute and solvent and the boiling point elevation, the molality can be calculated with m = (moles of solute) / (kilograms of solvent). The moles of solute is molar mass dependent, so when we rearrange to solve for molar mass, we get M = (mass of solute in grams) / (molality ⋅ kg of solvent).

To solve the problem, the steps are as follows:

Answer:

12.4×10^3 V

Explanation:

From E=hc/wavelength= eV

The voltage becomes

V= hc/e* wavelength

V= 6.63*10^-34*3*10^8/1.6*10^-19*1*10^-10

Note that the energy of the photon is transferred to the electron. That is the basic assumption we have applied in solving this problem. The kinetic energy of the electron is equal to the product of the electron charge and the acceleration potential.

1. The fraction of the atomic volume occupied by the nucleus is approximately 0.0000064 or 6.4 x 10^-6.

2. The density of a proton is approximately 5.77 x 10^20 g/cm^3.

Part 1: Fraction of atomic volume occupied by nucleus

**1. Calculate volumes of atom and nucleus:**

- Convert Å to m:

   - Atom diameter: 2.50 Å * 10^-10 m/Å = 2.50 x 10^-10 m

   - Nucleus diameter: 9.00 x 10^-5 Å * 10^-10 m/Å = 9.00 x 10^-15 m

- Calculate radii:

   - Atom radius: 2.50 x 10^-10 m / 2 = 1.25 x 10^-10 m

   - Nucleus radius: 9.00 x 10^-15 m / 2 = 4.50 x 10^-15 m

- Calculate volumes of spheres using the formula (4/3)πr³:

   - Atom volume: (4/3)π * (1.25 x 10^-10 m)³ ≈ 8.18 x 10^-31 m³

   - Nucleus volume: (4/3)π * (4.50 x 10^-15 m)³ ≈ 52.36 x 10^-44 m³

**2. Calculate fraction of volume occupied by nucleus:**

- Divide nucleus volume by atom volume:

   - Fraction = 52.36 x 10^-44 m³ / 8.18 x 10^-31 m³ ≈ 0.0000064

Therefore, the fraction of the atomic volume occupied by the nucleus is approximately 0.0000064 or 6.4 x 10^-6.

Part 2: Density of a proton

**1. Convert mass of proton to kg:**

- 1 amu = 1.66057 x 10^-27 kg

- Proton mass: 1.0073 amu * 1.66057 x 10^-27 kg/amu ≈ 1.6726 x 10^-27 kg

**2. Calculate volume of a proton from its diameter:**

- Proton radius: 1.72 x 10^-15 m / 2 = 8.60 x 10^-16 m

- Proton volume: (4/3)π * (8.60 x 10^-16 m)³ ≈ 2.90 x 10^-45 m³

**3. Calculate density:**

- Divide proton mass by its volume:

   - Density = 1.6726 x 10^-27 kg / 2.90 x 10^-45 m³ ≈ 5.77 x 10^17 kg/m³

**4. Convert density to g/cm^3:**

- 1 kg/m³ = 1000 g/cm³

- Density ≈ 5.77 x 10^17 kg/m³ * 1000 g/cm³ ≈ 5.77 x 10^20 g/cm³

Therefore, the density of a proton is approximately 5.77 x 10^20 g/cm^3.

The unit cell described is called the simple cubic unit cell, which contains one atom total due to each corner atom being shared by eight unit cells.

The name of the unit cell of the crystal lattice you've described is the simple cubic unit cell, also known as primitive cubic unit cell. In a simple cubic lattice, the unit cell that repeats itself in all directions to form the entire lattice is a cube with atoms at its corners. These atoms effectively 'touch' each other, and each corner atom is shared among eight unit cells; hence, each unit cell contains one-eighth of an atom at each of its eight corners, totaling one atom per unit cell.

Answer:

Since ΔEN > 0, the bond is covalent polar and the molecule is polar (dipole). Since ΔEN > 0, the bond is covalent polar and the molecule is polar (dipole). HI and ClF interact through a dipole-dipole force

Explanation:

Final answer:

Dipole-dipole forces act between a hydrogen chloride molecule and a hydrogen iodide molecule due to the partially positive hydrogen atom and partially negative chlorine atom in a hydrogen chloride molecule.

Explanation:

Dipole-dipole forces, which are attractive forces between polar molecules, act between a hydrogen chloride molecule and a hydrogen iodide molecule. These forces occur because a hydrogen chloride molecule has a partially positive hydrogen atom and a partially negative chlorine atom. In a collection of many hydrogen chloride molecules, the oppositely charged regions of neighboring molecules will align themselves near each other.

Answer:

For a: The charge on the ion formed is +3

For b: The charge on the ion formed is -2

For c: The charge on the ion formed is +2

Explanation:

An ion is formed when an atom looses or gains electron.

For the given options:

Aluminium is the 13th element of the periodic table having electronic configuration of [tex]1s^22s^22p^63s^23p^1[/tex]

This element will loose 3 electrons to form [tex]Al^{3+}[/tex] ion

The charge on the ion formed is +3

Sulfur is the 16th element of the periodic table having electronic configuration of [tex]1s^22s^22p^63s^23p^4[/tex]

This element will gain 2 electrons to form [tex]S^{2-}[/tex] ion

The charge on the ion formed is -2

Strontium is the 38th element of the periodic table having electronic configuration of [tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^2[/tex]

This element will loose 2 electrons to form [tex]Sr^{2+}[/tex] ion

The charge on the ion formed is +2

Glycine, an amino acid, changes its structure and net charge in response to pH due to two dissociable protons. At pH 2 it's fully protonated with a net charge of +1. At pH 7, its carboxyl group loses a proton leaving the net charge to 0. By pH 10, both the carboxyl and amino group have lost protons, so the net charge is -1.

The amino acid glycine (H2N–CH2–COOH) has two dissociable protons, one associated with its carboxyl group (pK 2.35) and one with its amino group (pK 9.78). At very low pH values, protons are abundant, meaning glycine is in its fully protonated form with a net charge of +1. Thus, at pH 2, the structure is H3N+–CH2–COOH and the net charge is +1.

At pH 7, the proton on the carboxyl group is lost, leaving the carboxylate form (COO-) and the proceed ammonium group (NH3+). Our structure therefore becomes H3N+–CH2–COO- with a net charge of zero.

Finally, at pH 10, glycine loses both of its protons. The structure now is H2N–CH2–COO- and the net charge is -1.

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Explanation:

When we move across a period from left to right then there will occur an increase in electronegativity and also there will occur an increase in non-metallic character of the elements.

As both arsenic (As) and antimony (Sb) are group 15 elements. And, on moving down the group increases metallic character hence, Sb will be more metallic than As. Therefore, As is less metallic in nature than Sb.  

Silicon (Si) is a group 14 element and phosphorus (P) is a group 15 element. And, both of them lie in period 3 and since, non-metallic character increases on moving from left to right along a period. Therefore, phosphorus (P) is less metallic than silicon (Si).    

Sodium (Na) is a group 1A element (also known as alkali metal) and beryllium (Be) is a group 2A element (also known as alkaline earth metal). Hence, Be is less metallic than Na because on moving from left to right there occurs an increase in non-metallic character.

Answer:

E) The rate of the reaction is directly proportional to the concentration of the reactant.

Explanation:

Give the characteristic of a first order reaction having only one reactant.

A) The rate of the reaction is not proportional to the concentration of the reactant.

B) The rate of the reaction is proportional to the square of the concentration of the reactant.

C) The rate of the reaction is proportional to the square root of the concentration of the reactant.

D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant.

E) The rate of the reaction is directly proportional to the concentration of the reactant.

Answer:

The rate of the reaction is directly proportional to the concentration of the reactant.

Explanation:

Answer:

0.144 M

Explanation:

First, we will calculate the mass/volume percent (% m/v) using the following expression.

% m/v = % m/m × density

% m/v = 2.50 % × 1.04 g/cm³

% m/v = 2.60 %

This means that there are 2.60 grams of solute per 100 cm³ (100 mL) of solution. The molarity of glucose is:

M = mass of glucose / molar mass of glucose × liters of solution

M = 2.60 g / 180.16 g/mol × 0.100 L

M = 0.144 M

Explanation:

Formula according to the radius ratio rule is as follows.

             [tex]\frac{r_{+}}{r_{-}} = \frac{73}{184}[/tex]

                          = 0.397

According to the radius ratio rule, as the calculated value is 0.397 and it lies in between 0.225 to 0.414. Therefore, it means that the type of void is tetrahedral.

Thus, we can conclude that the given compound is most likely to adopt closest-packed array with lithium ions occupying tetrahedral holes.

Answer:

closest-packed array with lithium ions occupying tetrahedral holes

Explanation:

Given the small size of lithium ions and that they are present in twice the amount as selenide ions, they must occupy tetrahedral holes in a closest-packed array.

The 2p sublevel has quantum numbers n=2, l=1, and possible ml values of -1, 0, +1, with a maximum of 6 electrons. The 5f sublevel has quantum numbers n=5, l=3, and possible ml values ranging from -3 to +3, holding up to 14 electrons.

The n, l, and possible ml values for 2p and 5f sublevels are derived from the quantum numbers that define the properties of electrons in atoms. For the 2p sublevel, n is 2 (the principal quantum number indicating the second shell), l is 1 (the angular momentum quantum number corresponding to a p sublevel), and the possible ml values range from -1 to +1 (which are -1, 0, and 1), making for three possible orientations.

For the 5f sublevel, n is 5 (indicating the fifth shell), l is 3 (f sublevel), and the possible ml values range from -3 to +3 (which are -3, -2, -1, 0, 1, 2, 3), resulting in a total of seven possible orientations. Using the formula maximum number of electrons that can be in a subshell = 2(2l + 1), we can calculate that the 2p sublevel can hold a maximum of 6 electrons and the 5f sublevel can hold up to 14 electrons.