When oxygen is depleted, the citric acid cycle stops. What could we add to the system to restore citric acid cycle activity (other than oxygen)?

Answer:

6) For 0.04392 moles BaSO4 we need 0.02196 moles Na2SO4

To produce 0.02196 moles Ba2SO4 and 0.04392 moles Na2SO4

7)  For 16.08 moles LiOH we'll have 8.04 moles H2SO4 produced.

We need 8.04 moles Li2SO4 and 8.04 moles H2O

8) For 0.0206 moles silvernitrate we'll hace 0.0206 moles silver

9) For 0.014 moles of Cu we'll have 0.014 moles Cu(NO3)2

Explanation:

6. Barium sulfate and and sodium sulfate react in a double displacement reaction. If the  reaction starts with 10.25 grams of barium sulfate what are the products and how many moles  of each product is produced?

Step 1: Data given

Mass of BaSO4 = 10.25 grams

Molar mass = 233.38 g/mol

Step 2: The balanced equation

2BaSO4 + Na2SO4 → Ba2SO4 + 2NaSO4

Step 3: Calcuate moles BaSO4

Moles BaSO4 = 10.25 grams / 233.38 g/mol

Moles BaSO4 = 0.04392 moles BaSO4

Step 4: Calculate moles

For 2 moles BaSO4 we need 1 mol Na2SO4 to produce 1 mol Ba2SO4 and 2 moles NaSO4

For 0.04392 moles BaSO4 we need 0.04392/2 = 0.02196 moles Na2SO4

To produce 0.02196 moles Ba2SO4 and 0.04392 moles Na2SO4

7. Calculate the moles of Li2SO4that would be needed to produce 385 g of LiOH.

Step 1: Data given

Mass of LiOH = 385 grams

Molar mass of LiOH = 23.95 g/mol

Step 2: The balanced equation

Li2SO4 + 2H2O → 2LiOH + H2SO4

Step 3: Calculate moles LiOH

Moles LiOH = 385.0 grams / 23.95 g/mol

Moles LiOH = 16.08 moles LiOH

Step 4: Calculate moles

For 1 mol Li2SO4 we need 2 moles H2O to produce 2 moles LiOH and 1 mol H2SO4

For 16.08 moles LiOH we'll have 8.04 moles H2SO4 produced.

We need 8.04 moles Li2SO4 and 8.04 moles H2O

8. Silver nitrate reacts with copper in a single displacement reaction. To produce copper (1) nitrate and silver. If 3.50 g of silver nitrate are reacted with excess copper. How many mole of  silver would be produced?

Step 1: Data given

Mass of AgNO3 = 3.50 grams

Molar mass of AgNO3 = 169.87 g/mol

Step 2: The balanced equation

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

Step 3: Calculate moles AgNO3

Moles AgNO3 = 3.50 grams / 169.87 g/mol

Moles AgNO3 = 0.0206 moles

Step 4: Calculate moles of Ag

For 1 mol copper, we need 2 moles of silvernitrate to produce 1 mol of coppernitrate and 2 moles of silver

For 0.0206 moles silvernitrate we'll hace 0.0206 moles silver

9. (Use the chemical equation from above) How many moles of copper (1) nitrate ]can be  produced with and 0.89 grams of copper metal?

Step 1: Data given

Mass of Cu = 0.89 grams

Molar mass of Cu = 63.55 g/mol

Step 2: The balanced equation

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

Step 3: Calculate moles Cu

Moles Cu =0.89 grams / 63.55 g/mol

Moles Cu = 0.014 moles

Step 4: Calculate moles of Coppernitrate

For 1 mol copper, we need 2 moles of silvernitrate to produce 1 mol of coppernitrate and 2 moles of silver

For 0.014 moles of Cu we'll have 0.014 moles Cu(NO3)2

Answer: C) Non-metals can share pairs of electrons and form covalent bonds

Explanation: The principal reason why it is non-metals that can form covalent bonds is because of their electronegativities. Electronegativity is the tendency of an atom to attract electrons towards itself.

The participating atoms in a covalent bond have to be able to hold the shared electron in place & it is this attraction towards the centre of each participating atom that holds the electrons in place. Metals aren't electronegative, they don't attract electrons towards each other, they'd rather even push the electrons away from themselves (electropositive) to be stable. The closest concept of metals to shared electrons is in metallic bonding, where metals push and donate their valence electrons to an electron cloud which is free to move around the bulk of the metallic structure. But this is nowhere near the type of bonding that exist in covalent bonds.

Answer:

C) Nonmetals can share pairs of electrons and form covalent bonds.

Explanation:

Answer:

72.53% is the yield of CrCl3

Explanation:

Given

Reaction:

Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)

CCl4 is in excess and 17.6g  Cr2O3 present

The reaction yields 26.6g of CrCl3

To Find:

% yields of the reaction

Also given

Molar mass of CrCl3 = 158.35g/mol

Molar mass of Cr2O3 = 152.00 g/mol

By the stoichiometry of the reaction

1 mole of Cr2O3 gives  2 moles of CrCl3

0r

1 x1 52 g of Cr2O3 gives 2x 158.35 g of CrCl3

= 1 52 g of Cr2O3 gives 316.70 g of CrCl3

    17.6 g of Cr2O3 gives  (17.6÷152) × 316.70 g CrCl3

= 36.67 g CrCl3

but actual yield is only 26.6g

so % yield is (26.6 ÷÷ 36.67) × 100

= 72.53% is the yield of CrCl3

Final answer:

To calculate the percent yield, the number of moles of chromium(III) oxide used was first determined, which was then used to find the theoretical yield of chromium chloride. The actual yield of chromium chloride is compared to this theoretical yield to find that the percent yield of the reaction is approximately 72.48%.

Explanation:

The student asked to calculate the percent yield of a chemical reaction involving chromium(III) oxide (Cr2O3) and carbon tetrachloride (CCl4). To find the percent yield, we need to compare the actual yield to the theoretical yield. First, we calculate the number of moles of Cr2O3 that react. With a molar mass of 152.00 g/mol, 17.6 g of Cr2O3 is equivalent to 0.1158 moles. According to the stoichiometry of the balanced equation, 1 mole of Cr2O3 produces 2 moles of CrCl3, which suggests that 0.1158 moles of Cr2O3 would yield 0.2316 moles of CrCl3. Using the molar mass of CrCl3 (158.35 g/mol), the theoretical yield of CrCl3 can be found as 0.2316 moles × 158.35 g/mol = 36.7 g.

Now, we calculate the percent yield using the actual yield (26.6 g) and the theoretical yield (36.7 g).

Percent Yield = (Actual Yield / Theoretical Yield) × 100 = (26.6 g / 36.7 g) × 100 ≈ 72.48%

Therefore, the percent yield of chromium chloride in the reaction is approximately 72.48%.

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle.

This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

Increase the volume:

If the volume of the container is increased, the pressure will decrease according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where increase in pressure is taking place. So, the equilibrium will shift in a direction where more number gaseous moles are present.

A) [tex]2COF_2(g)\rightleftharpoons CO_2(g)+CF_4(g)[/tex]

Number of gaseous moles on reactant side = 2

Number of gaseous moles on product side = 2

Equilibrium will not shift any direction as on both sides number of gaseous moles are same.

B) [tex]2NO(g)+O_2(g)\rightleftharpoons 2NO_2(g)[/tex]

Number of gaseous moles on reactant side = 3

Number of gaseous moles on product side = 2

Equilibrium will shift any left direction.

C) [tex]2N_2O_5(g)\rightleftharpoons 4NO_2(g)+O_2[/tex]

Number of gaseous moles on reactant side = 2

Number of gaseous moles on product side = 5

Equilibrium will shift any right direction.

D) [tex]2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)[/tex]

Number of gaseous moles on reactant side = 3

Number of gaseous moles on product side = 2

Equilibrium will shift any left direction.

E) [tex]PCl_5\rightleftharpoons PCl_3(g)+Cl_2(g)[/tex]

Number of gaseous moles on reactant side = 1

Number of gaseous moles on product side = 2

Equilibrium will shift any right direction.

Answer:

Proton: m= 1.6726x10⁻²⁷ kg

Neutron: m= 1.6749x10⁻²⁷ kg

Electron: m= 9.1164x10⁻³¹ kg

Explanation:

We can calculate the mass of a proton, neutron, and electron using the following data:

mass of proton: 1.00728 amu

mass of neutron: 1.00867 amu

mass of electron: 5.49x10⁻⁴ amu

1 amu = 1.66054x10⁻²⁷ kg

Now, the mass of a proton, neutron, and electron in kilograms can be calculated using the next relation:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot particle's mass (amu) [/tex]

For the proton:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00728 amu = 1.6726 \cdot 10^{-27} kg [/tex]

For the neutron:    

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00867 amu = 1.6749 \cdot 10^{-27} kg [/tex]

For the electron:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 5.49x10⁻⁴ amu = 9.1164 \cdot 10^{-31} kg [/tex]    

I hope it helps you!

The masses of proton, neutron, and electron are approximately 1.6726 x 10-27 kg, 1.6749 x 10-27 kg and 9.109 x 10-31 kg, respectively. This is calculated by multiplying each particle's mass in Atomic Mass Units by the factor 1.66054 × 10-27 kg/amu.

To calculate the mass of a proton, neutron, and electron in kilograms, we must know their masses in Atomic Mass Units (amu). We know that 1 amu = 1.66054 × 10

-27 kg. Using this we can get the masses as:

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Answer:

a) 0.67 moles of O2

b) 1.34 moles H2O

c) 24.15 grams of H2O

d) 21.44 grams O2

Explanation:

Step 1: Data given

Dihydrogen dioxide = H2O2

oxygen gas = O2

Moles H2O2 = 1.34 moles

Molar mass of H2O2 = 34.01 g/mol

Step 2: The balanced equation

2H2O2 → 2H2O + O2

Step 3: Calculate moles of H2O formed

For 2 moles H2O2 we'll have 2 moles H2O produced

For 1.34 moles H2O2 we have 1.34 moles H2O produced

This is 1.34 moles * 18.02 g/mol = 24.15 grams of H2O

Step 4: Calculate moles of O2 formed

For 2 moles H2O2 we'll have 1 mol O2 produced

For 1.34 moles H2O2 we'll have 1.34 /2 = 0.67 moles of O2 produced

This is 0.67 moles * 32.00 g/mol = 21.44 grams O2

HF and CH3OH exhibit dipole-dipole forces when dissolved in water because they both can form hydrogen bonds. CaCl2 and FeBr3 display ion-dipole forces in water because they are ionic compounds.

When these substances are added to water, they exhibit different solute-solvent interactions due to their different properties.

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Answer:

c.Baking Soda (sodium bicarbonate)

Explanation:

The Arrhenius theory was introduced introduced by Swedish scientist named Svante Arrhenius in 1887.

According to the theory, acids are the substances which dissociate in the aqueous medium to produce electrically charged atoms ( may be molecule). Out of these species furnished, one must be a proton or the hydrogen ion, [tex]H^+[/tex].

Base are the substances which dissociate in the aqueous medium to produce electrically charged atoms ( may be molecule). Out of these species furnished, one must be a hydroxide ion, [tex]OH^-[/tex].

a. Lemon juice contains citric acid which is an acid.

b. Vinegar contains acetic acid which is an acid.

c. Baking Soda contains sodium bicarbonate and is a base.

Thus, c is the answer.

pH is defined as the negative logarithm of the concentration of hydrogen ions.

Thus,  

pH = - log [H⁺]

pH scale generally runs from 1 to 14 where pH = 7 represents neutral medium, pH < 7 represents acidic medium and pH > 7 represents basic medium.

d. Substance with pH 7 represents neutral solution.

Answer:

224 grams of O₂

Explanation:

This is the reaction:

2 C₂H₆ (g) + 7 O₂(g) → 4 CO₂ (g) + 6 H₂O (g)

2 moles of ethene react with 7 moles of oxygen.

Let's convert the ethene's mass into moles (mass / molar mass)

60 g / 30 g/m = 2 mol

So, if 2 moles of ethene must react with 7 moles of O₂ and we have 2 moles, obviously we would need 7 moles of oyxgen.

Let's convert the moles to mass ( mol . molar mass)

7 m . 32 g/m = 224 grams

Answer: Mass of O2 is 224g

Explanation:

From the equation of the reaction, Ethane to oxygen is 2 to 7

While the molar masses respectively gives 30 and 32 g/mol

2 moles of methane gives 7 moles of O2;

60g/30=2moles for methane gives x/32 for O2;

Cross multiplying yields

7 x 2 = 2 x mass of O2/32

14 = 2x/32

Final answer gives 224 grams of oxygen

Answer:

Oxidation process

Explanation:

Oxidation is the transfer of electrons from an atom, molecule, or ion to another atom, molecule, or ion in a chemical reaction.

Oxidation is said to have taken place when the oxidation status of a atom, molecule, or ion is increases.

Oxidation process is said to include

Addition of oxygen atom or Electronegative atoms to another atom, molecule, or ion

Loss of one or more electrons by a atom, molecule, or ion

Increase in the oxidation number of a atom, molecule, or ion

Loss of a hydrogen or Electropositive atoms

Answer:

Carbon Dioxide is an Infrared Radiation Absorber. The (CO2) molecules also emits the absorbed infrared (IR) radiation energy. The photon energy from the infrared radiation causes the CO2 molecule to vibrate. Only some of its vibrational modes absorb infrared radiation

Explanation:

Its linear structure is considered when working with the formula to calculate the number of molecular vibrational modes. It has 3n - 4 vibrational modes, where n is the number of atoms in a compound of CO2

With 3 atoms, CO2 has

3n−5=4 types or patterns of vibration

1. The symmetric stretch

2. The asymmetric stretch

3. The bend

The symmetric stretch vibrational mode is ir-inactive.

The asymmetric stretch is ir-active as it results in changes in dipole moment

The bend is ir-active as well as it results in a change in dipole moment too.

At the molecular level as the CO2 molecules absorb photons of the infrared radiation, the atoms in the CO2 molecules increase their vibration as the bonds between the atoms bend and stretch.

The question is incomplete, the complete question is;

The infrared spectrum above represents the absorption of certain wavelengths of radiation by molecules of CO2. Which of the following best explains what occurs at the molecular level as the CO2 molecules absorb photons of the infrared radiation?

The infrared spectrum of molecules is based on changes in the vibrational energy levels within the molecule.

Infrared radiation causes bonds to vibrate. The nature of the vibration may be stretching or bending.

So, when CO2  molecules are irradiated with infrared radiation, at the molecular level, CO2 molecules absorb photons of the infrared radiation, the atoms in the CO2 molecules increase their vibration as the bonds between the atoms bend and stretch.

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Answer:

Gastric juices have a pH of 1 or 2. This would indicate numerous H+ ions and a low pH

Explanation:

Highers concentrations of [H⁺] means very low pH.

pH = - log [H⁺]

Imagine this two concentrations:

[H⁺]₁ = 0.2 M

[H⁺]₂ = 0.0006 M

[H⁺]₁ > [H⁺]₂

pH₁ = - log 0.2 → 0.70

pH₂ = - log 0.0006 → 3.22

Then pOH₁ = 14 - 0.70 = 13.30

pOH₂ = 14 - 3.22 = 10.78

[OH⁻]₁ = 10^-pOH = 5.01×10⁻¹⁴

[OH⁻]₂ = 10^-pOH = 1.66×10⁻¹¹

As pH is so low, [OH⁻] is more and more lower.

Answer:

The solution needs to remain hot during filtration in order to remove impurities and charcoal that are insoluble in the crystallization solvent, also to prevent crystals form prematurely on the paper filter or on the funnel stem.

Answer:

The balanced redox is:

14 H⁺ + Cr₂O₇²⁻ + 3Sn²⁺ → 3Sn4⁺  + 2Cr³⁺  + 7H₂O

So the coefficient for the H⁺ is greater than 4 (option E)

Explanation:

This is the redox reaction:

Cr₂O₇²⁻ (aq) + Sn²⁺ (aq)  →  Cr³⁺ (aq) + Sn⁴⁺(aq)

First of all, we must determine the half reactions:

In dycromate, Cr acts with +6 in the oxidation state → Cr cation has +3 in product side - Oxidation state, has decreased so this is the reduction.

In reactant side Sn cation acts with +2 → In product side Sn acts with +4

The oxidation state has increased, so this is the oxidation.

Cr₂O₇²⁻  → Cr³⁺

We have to add 2, to Cr in reactant side, and as we are in adicid medium we add water in the opposite side of oxygen. The same amount of oxgen, that we have.

Cr₂O₇²⁻  → 2Cr³⁺ + 7H₂O

Finally, as we have 14 H in product side, we must add 14 H⁺ to the reactant side. Cr+⁶ in dycromate to change to Cr³⁺, gained 3 e⁻, but we have 2 Cr, so in total the Cr gained 6e⁻. The balanced half reaction is:

14 H⁺ + Cr₂O₇²⁻ + 6e⁻ → 2Cr³⁺  + 7H₂O

Sn²⁺ to change the oxidation state, to +4 had to release electrons:

Sn²⁺ →  Sn4⁺  + 2e⁻

The electrons are unbalanced, so we must to multiply the half reactions:

(14 H⁺ + Cr₂O₇²⁻ + 6e⁻ → 2Cr³⁺  + 7H₂O) x1

(Sn²⁺ →  Sn4⁺  + 2e⁻ ) x3

And we sum both:

14 H⁺ + Cr₂O₇²⁻ + 6e⁻ + 3Sn²⁺ → 3Sn4⁺  + 6e⁻  + 2Cr³⁺  + 7H₂O

To balance the redox equation in acidic solution, follow these steps: Write the unbalanced equation, identify the oxidation and reduction half-reactions, balance the atoms and charges, multiply the oxidation half-reaction, combine the half-reactions, and balance the equation by dividing through by common factors. The correct coefficient for the H+ ion is 2.

To balance the redox equation in acidic solution, we need to follow these steps:

Upon balancing the equation, we find that the correct coefficient for the H+ ion is (B) 2.

Answer:

2.3x10⁷ W/m²

Explanation:

The intensity (I) of a laser is its potency (P) divided by the area (A) that it is affected. The potency is the energy applied (or absorbed) in a period, thus id 91.0% of the energy is absorbed, so:

E = 0.91*540 = 491.4 J

And,

P = E/t, where t is the time in seconds

P = 491.4/4.00

P = 122.85 J/s

P = 122.85 W

The are of a circular spot is:

A = (π/4)*d²

Where d is the diameter. Thus, with d = 2.60 mm = 0.0026 m

A = (π/4)*(0.0026)²

A = 5.31x10⁻⁶ m²

I = P/A

I = 122.85/5.31x10⁻⁶

I = 2.3x10⁷ W/m²

Answer:

4. 1; 6; 2 — synthesis

Explanation:

Decomposition reaction is defined as the reaction in which a single large substance breaks down into two or more smaller substances.

[tex]AB\rightarrow A+B[/tex]

Single displacement reaction is defined as the reaction in which more reactive element displaces a less reactive element from its chemical reaction.

The reactivity of metal is determined by a series known as reactivity series. The metals lying above in the series are more reactive than the metals which lie below in the series.

[tex]A+BC\rightarrow AC+B[/tex]

Synthesis reaction is defined as the reaction in which smaller substances combine in their elemental state to form a larger substance.

[tex]A+B\rightarrow AB[/tex]

The unbalanced combustion reaction is shown below as:-

[tex]P_4+Ca\rightarrow Ca_3P_2[/tex]

On the left hand side,  

There are 4 phosphorus atoms and 1 calcium atom

On the right hand side,  

There are 2 phosphorus atoms and 3 calcium atoms

Thus,  

Right side, [tex]Ca_3P_2[/tex] must be multiplied by 2 to balance phosphorus.

Left side, [tex]Ca[/tex] is multiplied by 6 so to balance the whole reaction.

Thus, the balanced reaction is:-

[tex]P_4+6Ca\rightarrow 2Ca_3P_2[/tex]

Thus, answer:- 4. 1; 6; 2 — synthesis

The atomic mass of gallium if gallium has two naturally occurring isotopes with the following masses and natural abundances: Ga-69, 68.9256 amu 60.1%, and Ga-71, 70.9247 amu 39.9%, is 69.7376073 amu. Hence, option d is the correct answer.

Given the isotopes and their masses and abundances:

Ga-69 with a mass of 68.9256 amu and an abundance of 60.1%.

Ga-71 with a mass of 70.9247 amu and an abundance of 39.9%.

Atomic mass ([tex]M_a_t_o_m_i_c[/tex]) using the formula.

[tex]M_a_t_o_m_i_c[/tex]=([tex]M_i_s_o_t_o_p_e_1[/tex] ×abundance1)+([tex]M_i_s_o_t_o_p_e_2[/tex]×abundance2)

[tex]M_a_t_o_m_i_c[/tex]=(68.9256amu×0.601)+(70.9247amu×0.399)

[tex]M_a_t_o_m_i_c[/tex]=41.413512amu+28.3240953amu

[tex]M_a_t_o_m_i_c[/tex]=69.7376073amu

Rounded to the nearest hundredth, the calculated atomic mass of gallium is approximately 69.73 amu. The closest option is "d that is 69.7 amu," which is approximately the same as the calculated atomic mass of gallium. Hence, option d is the correct answer.

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The atomic mass of gallium, considering its two naturally occurring isotopes, Ga-69 and Ga-71, with masses of 68.9256 amu and 70.9247 amu at abundances of 60.11% and 39.89% respectively, is approximately 69.7171 amu.

The atomic mass of an element is calculated considering all its naturally occurring isotopes. In this case, gallium has two stable isotopes, Ga-69 and Ga-71, with respective masses and natural abundances stated in the question. Here are the steps to calculate the atomic mass of gallium:

Firstly, we multiply the mass of each isotope by its natural abundance:

For Ga-69:

68.9256 amu * 60.11 / 100 = 41.4292 amu

For Ga-71:

70.9247 amu * 39.89 / 100 = 28.2879 amu

Then, we add the results to get the atomic mass:

41.4292 amu + 28.2879 amu = 69.7171 amu

So, the atomic mass of gallium is approximately 69.7171 amu.

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Answer:

Explanation:

Because most of the volume occupied by the substance is empty space.

Answer:

Mg₃N₂ + 6H₂O  →  2NH₃  +  3Mg(OH)₂

Coefficient of water is 6 (option 3)

Explanation:

The reaction is:

Mg₃N₂ + H₂O  →  NH₃  +  Mg(OH)₂

Let's balance the reaction.

In reactant side we have 3 Mg, therefore in product side, we add 3 Mg to the hydroxide.

This change, modified the hydroxide, so now we have 6 O and 6 H, but we have in total 9 H (6 from the hydroxide + 3 from the ammonia)

As we have 2N, in reactant side, we must add 2 N to the ammonia, so now

we have 12 H in product side . We must complete with 6, the water so the H are ballanced.

In reactant side we have 6 O, therefore in product we must have 6 O (two O, in the OH but we have 3 moles, so in total we have 6 O) - BALANCED

The balance reaction is:

Mg₃N₂ + 6H₂O  →  2NH₃  +  3Mg(OH)₂

The chemical reaction of magnesium nitride with water to form ammonia and magnesium hydroxide has a coefficient of 6 for water in the balanced equation.

Preparing ammonia through the reaction of magnesium nitride with water yields ammonia and magnesium hydroxide. The balanced chemical equation for this reaction is: Mg3N2 + 6H2O → 3NH3 + 3Mg(OH)2. Thus, the coefficient of water in the balanced chemical equation is 6, which corresponds to option number 3 in your question.

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Answer:

1. Reduce

2. Oxidize

3. Oxidize

4. Reduce

5. Oxidize

6. Reduce

Explanation:

Answer:

1. Reduce, Oxidize

2.Oxidize, reduce

3.Reduce, Oxidize

Explanation:

Answer:

Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside.

Explanation:

Sodium ion and potassium ion play an important role in cellular metabolism. Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

Sodium ions are necessary for:

generation of nerve impulse

Heart activities

electrolyte balance

High or low concentration of sodium affects health.

Potassium ions are necessary for:

fluid and electrolyte balance

Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

Therefore, Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

The correct statement is that Na+ is the most plentiful positively charged ion outside the cell, while K+ is more plentiful inside, due to the function of the sodium-potassium pump in the plasma membrane of cells.

The statement that is true among the given options is: Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside. This arrangement is made possible through a process called the sodium-potassium pump, which is part of the plasma membrane of cells. The pump uses ATP to move 3 Na+ out of the cell and 2 K+ into the cell, which helps maintain the cell's resting potential. Therefore, outside of the cells, there is a higher concentration of Na+ ions, while inside the cells, K+ ions are more plentiful.

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Answer:

10.1 g of Al are formed

Explanation:

The reaction is:

2AlCl3 --> 2Al + 3Cl2

So 2 moles of aluminun chloride decompose into 2 moles of Al and 3 moles of chlorine.

Ratio is 2:2.

Let's convert the mass of salt into moles (mass / molar mass)

50 g / 133.34 g/mol = 0.374 moles.

As the ratio is 2: 2, if I have 0.374 moles of salt, I would produce the same amount of Al, just 0.374.

Let's convert the moles to mass

(Mol . molar mass)

0.374 mol . 26.98 g / mol = 10.1 g of Al are formed

Ξ

28.99 grams of aluminium metal can be produced when 50.0 grams of aluminium chloride decompose.

To solve this problem, we will use stoichiometry, which involves the following steps:

1. Write down the balanced chemical equation:

[tex]\[ 2\text{AlCl}_3 \rightarrow 2\text{Al} + 3\text{Cl}_2 \][/tex]

2. Calculate the molar mass of aluminium chloride (AlCl3) and aluminium (Al):

- The molar mass of Al is approximately 26.98 g/mol.

- The molar mass of AlCl3 is calculated as follows:

[tex]\[ \text{Molar mass of AlCl}_3 = \text{Molar mass of Al} + 3 \times \text{Molar mass of Cl} \] \[ \text{Molar mass of AlCl}_3 = 26.98 \text{ g/mol} + 3 \times 35.45 \text{ g/mol} \] \[ \text{Molar mass of AlCl}_3 = 26.98 \text{ g/mol} + 106.35 \text{ g/mol} \] \[ \text{Molar mass of AlCl}_3 = 133.33 \text{ g/mol} \][/tex]

3. Convert the mass of AlCl3 to moles:

[tex]\[ \text{Moles of AlCl}_3 = \frac{\text{Mass of AlCl}_3}{\text{Molar mass of AlCl}_3} \] \[ \text{Moles of AlCl}_3 = \frac{50.0 \text{ g}}{133.33 \text{ g/mol}} \] \[ \text{Moles of AlCl}_3 \approx 0.375 \text{ mol} \][/tex]

4. Use the stoichiometric ratio from the balanced equation to find the moles of Al produced:

The balanced equation shows that 2 moles of AlCl3 produce 2 moles of Al. Therefore, the moles of Al produced are the same as the moles of AlCl3 that decomposed, since the ratio is 1:1.

5. Convert the moles of Al to grams:

[tex]\[ \text{Mass of Al} = \text{Moles of Al} \times \text{Molar mass of Al} \] \[ \text{Mass of Al} = 0.375 \text{ mol} \times 26.98 \text{ g/mol} \] \[ \text{Mass of Al} \approx 9.969 \text{ g} \][/tex]

However, since the stoichiometry of the reaction gives us 2 moles of Al for every 2 moles of AlCl3, we must account for this in our mass calculation. Therefore, we multiply the mass of Al by the ratio of the moles of Al produced to the moles of AlCl3 that reacted:

[tex]\[ \text{Mass of Al} = 9.969 \text{ g} \times \frac{2 \text{ mol Al}}{2 \text{ mol AlCl}_3} \] \[ \text{Mass of Al} = 9.969 \text{ g} \times 1 \] \[ \text{Mass of Al} \approx 9.969 \text{ g} \][/tex]

Since the stoichiometry does not change the mass calculation (because the ratio is 1:1 for Al and AlCl3), the mass of Al produced is approximately 9.969 grams. However, this is not the final answer, as we need to consider significant figures.

6. Round the final answer to the appropriate number of significant figures, which in this case is three (since the mass of AlCl3 is given to three significant figures):

[tex]\[ \text{Mass of Al} \approx 10.0 \text{ g} \][/tex]

However, upon re-evaluating the calculation, it seems there was a mistake in the conversion of moles of AlCl3 to moles of Al. Since the stoichiometry is 2 moles of AlCl3 to 2 moles of Al, the moles of Al should be equal to the moles of AlCl3, which is 0.375 moles. Therefore, the correct mass of Al is calculated as follows:

[tex]\[ \text{Mass of Al} = 0.375 \text{ mol} \times 26.98 \text{ g/mol} \] \[ \text{Mass of Al} = 28.985 \text{ g} \][/tex]

Rounding to three significant figures, we get:

[tex]\[ \text{Mass of Al} \approx 28.99 \text{ g} \][/tex]

Answer:

The answer is D

Explanation:

Law of Definite Proportions states that a given compound always contain its component elements in fixed ratio (by mass) and does not depend on its source and/or method of preparation.  

If one is to explain the law of definite proportions properly, then Dalton's fourth atomic theory comes to mind which states that atoms chemically combine with other atoms in fixed, whole number ratios.

The law of definite proportions suggests that compounds always contain its component elements in fixed ratio no matter the source, for example, oxygen makes up 8/9 of the mass of the sample of pure water regardless of the source while hydrogen makes up the remaining 1/9 of the mass. This generally shows that when oxygen and hydrogen combine in the ratio 8:1, water molecule will be formed as suggested by the Dalton Atomic Theory.

The Dalton's atomic theory postulate explaining the Law of Definite Proportions is 'Atoms chemically combine with other atoms in fixed, whole-number ratios.' This principle underlies consistent elemental proportions in compounds, such as the 1:8 ratio of hydrogen to oxygen in water.

The postulate of Dalton's atomic theory that is vital to explain the observations summarized by the Law of Definite Proportions is: 'Atoms chemically combine with other atoms in fixed, whole-number ratios.'

This is crucial because the Law of Definite Proportions states that a given compound, regardless of the source or preparation method, will always consist of the same elements in the same proportion by mass.

For example, water (H2O) is always composed of 2 hydrogen atoms and 1 oxygen atom (fixed, whole-number ratio) regardless of the source. In water, the ratio of the mass of hydrogen to oxygen is always 1:8, which corroborates the Law of Definite Proportions.

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Answer: 2,625.3 g AlCl3

Explanation: solution attached:

First balance the chemical equation then do basic stoichiometry.

Answer: B

Double replacement reaction

Explanation:

Answer:

sorry i cant read sideways

Explanation:

From what we have below, we can see the complete and full question.

Chlorofluorocarbons (CFCs) such as CF2Cl2 are refrigerants whose use has been phased out because of their destructive effect on Earth's ozone layer. The standard enthalpy of evaporation of CF2Cl2 is 17.4 kJ/mol, compared with delta Hvaporization = 41 kJ/mol for liquid water. How many grams of liquid CF2Cl2 are needed to cool 122.1 g of water from 48.6 to 27.6 degrees Celsius? The specific heat of water is 4.184 J/(g x degrees Celsius).

Answer:

74.56 g

Explanation:

Given that;

The standard enthalpy of evaporation of CF₂Cl₂ = 17.4 kJ/mol

Δ [tex]H_{vapourization}[/tex] = 41kJ/mol (for liquid water)

grams of liquid CF₂Cl₂ (i.e Mass of CF₂Cl₂ required to absorb the heat from water) = ???

mass( in gram) of water = 122.1g

Temperature (T₁) = 48.6°C

Temperature (T₂) = 27.6°C

ΔT = (T₂ - T₁) = 27.6° - 48.6° = -21°C

Specific heat of water (C) = 4.18 J/g*deg*°C

From the parameters given, let's first find and decide the quantity of heat absorbed from the given amount of water in the system.

Q (quantity of heat) = mCΔT

= 122.1 g × 4.18 J/g*deg*°C × 27.6°C

= -10728.1944 J

= -10.73 kJ

∴ -10.73 kJ is the amount of heat given to CF₂Cl₂ by the water.

NOTE: The negative sign illustrate the heat given by the water in the system)

Since that is  known, we can easily find the mass of CF₂Cl₂ needed to cool 122.1 g of water.

Since the molar mass of  CF₂Cl₂ = 120.91 g /mol

∴ Mass of CF₂Cl₂  needed to cool 122.1g of water = [tex]\frac{10.73kJ}{17.4kJ}*120.91g)

= 74.56g

Answer:

The answer is (B) A gamma ray alone

Explanation:

Technetium-99m decays through a process called isomeric transition involving the decay of 99mTc to 99TC via the release of gamma rays and low energy electron

Answer: The final pressure in the vessel will be 0.965 atm

Explanation:

To calculate the number of moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]      .....(1)

Given mass of phosphorus trichloride = 20.0 g

Molar mass of phosphorus trichloride = 137.3 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol[/tex]

Given mass of oxygen gas = 3.15 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol[/tex]

The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:

[tex]2PCl_3+O_2\rightarrow 2POCl_3[/tex]

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas

So, 0.146 moles of phosphorus trichloride will react with = [tex]\frac{1}{2}\times 0.146=0.073mol[/tex] of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride produces 2 moles of [tex]POCl_3[/tex]

So, 0.146 moles of phosphorus trichloride will produce = [tex]\frac{2}{2}\times 0.146=0.146mol[/tex] of [tex]POCl_3[/tex]

To calculate the pressure of the vessel, we use the equation given by ideal gas follows:

[tex]PV=nRT[/tex]

where,

P = pressure of the vessel = ?

V = Volume of the vessel = 6.00 L

T = Temperature of the vessel = [tex]210^oC=[210+273]K=483K[/tex]

R = Gas constant = [tex]0.0821\text{ L. atm }mol^{-1}K^{-1}[/tex]

n = number of moles = 0.146 moles

Putting values in above equation, we get:

[tex]P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm[/tex]

Hence, the final pressure in the vessel will be 0.965 atm

Answer:

The final pressure in the vessel is 1.13 atm

Explanation:

Step 1: Data given

Volume of the vessel = 6.00 L

Mass of PCl3 = 20.0 grams

Mass of O2 = 3.15 grams

Temperature = 15.0 °C

The vessel is heated to 210°C

Molar mass of PCl3 = 137.33 g/mol

Step 2: The balanced equation

2PCl3 + O2 → 2POCl3

Step 3: Calculate moles PCl3

MolesPCl3 = mass PCl3 / molar mass PCl3

Moles PCl3 = 20.0 grams / 137.33 g/mol

Moles PCl3 =0.146 moles PCl3

Step 4: Calculate moles O2

Moles O2 = 3.15 grams/ 32.0 g/mol

Moles O2 = 0.0984 moles O2

Step 5: Calculate the limiting reactant

PCl3 is the limiting reactant. It will completely be consumed(0.146 moles). So at completion there is no PCl3 remaining.

O2 is in excess. There will react 0.146/2 = 0.073 moles. There will remain 0.0984 - 0.073 = 0.0254 moles O2

Step 6: Calculate moles POCl3

For 2 moles PCl3 we need 1 mol O2 to produce 2 moles POCl3

For 0.146 moles PCl3 we'll have 0.146 moles POCl3

Step 7: Calculate final pressure

p*V = n*R*T

p = (n*R*T)/V

⇒ with n = the number of moles = 0.146 moles of POCl3 produced + 0.0254 moles O2 remaining = 0.1714 moles gas

⇒ with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 210 +273 = 483 Kelvin

⇒ with V = the volume = 6.00 L

p = (0.1714 *0.08206 * 483) / 6.00

p = 1.13 atm

The final pressure in the vessel is 1.13 atm

Answer:

He have higher pressure at room temperature.

Explanation:

It is given that both the gases are kept in 5 L chambers.

Therefore, volume is constant.

Also, they both are at room temperature, so temperature is also constant.

Now, number of moles of [tex]O_2[/tex] = [tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{32}=0.16\ mol.[/tex]

Also, number of moles of He =[tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{4}=1.25\ mol.[/tex]

Now, according to GAS LAW,

[tex]PV=nRT[/tex]  ( all terms have their usual meaning).

In this case, V, R and T are constant.

So, pressure is directly proportional to n i.e number of moles.

So, moles of He is more than moles of [tex]O_2[/tex].

Therefore, He have higher pressure at room temperature.

Hence , this is the required solution.

The gas that has a higher pressure is He.

Number of moles of oxygen gas = 5.00 g /32 g/mol = 0.156 moles

From PV = nRT

P = ?

V = 5 L

n =  0.156 moles

T = 25 + 273 = 298 K

R = 0.082 atmLK-1mol-1

P = nRT/V

P =  0.156 moles × 0.082 atmLK-1mol-1 × 298 K/5 L

P = 0.76 atm

Number of moles of He = 5/4 g/mol = 1.25 moles

P = ?

V = 5 L

n = 1.25 moles

T = 25 + 273 = 298 K

R = 0.082 atmLK-1mol-1

P = nRT/V

P =1.25 moles × 0.082 atmLK-1mol-1 × 298 K/5 L

P = 6.11 atm

The gas that has a higher pressure is He.

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