Question 1

Consider the reaction CO(g)+ 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

Accepted Answer

The decrease in the equilibrium constant (K) with an increase in temperature indicates that the reaction is exothermic. In exothermic reactions, increasing the temperature shifts the equilibrium towards the reactants, thus reducing the value of K.

Question 2

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction,$\Delta$HS1U1P1$\circ$S1S1P0 = 92.38 kJ.mol^-1.

Accepted Answer

The answer of For the decomposition of ammonia to nitrogen...

Question 3

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Accepted Answer

The answer of For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)]...

Question 4

Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

Accepted Answer

The equilibrium constant K is extremely large (10^80), indicating that the reaction proceeds almost completely to the right, converting nearly all reactants to products. Therefore, the concentration of ammonia at equilibrium is approximately 0 M.

Question 5

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Accepted Answer

The answer of For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K...

Question 6

Consider the reaction 4NH₃(g)+ 7O₂(g) →2N₂O₄(g)+ 6H₂O(g) If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

Accepted Answer

The answer of Consider the reaction 4NH₃(g)+ 7O₂(g) →2N₂O₄(g)+ 6H₂O(g) If,initially,[NH₃(g)] =...

Question 7

The equilibrium constant K for the dissociation of N₂O₄(g)to NO₂(g)is 1700 at 500 K.Predict its value at 300 K.For this reaction,$\Delta$HS1U1P1$\circ$S1S1P0 is 56.8 kJ.mol^-1.

Accepted Answer

The answer of The equilibrium constant K for the dissociation...

Question 8

Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

Accepted Answer

At equilibrium, the concentration of each species can be calculated using the equilibrium constant expression: K = [N₂]2[H₂O]6/[NH₃]4[O₂]3 Substituting the initial concentration of 12 M for each species, we can simplify the expression to: 10⁸⁰ = (2x)2(6x)6/ (12-4x)4(12-3x)3 where x is the change in concentration of oxygen at equilibrium. Solving for x using a numerical method such as the quadratic formula or a graphical method, we get x ≈ 3 M. Therefore, the approximate concentration of oxygen at equilibrium is 3 M.

Question 9

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

Accepted Answer

The answer of If the equilibrium constant for the reaction...

Question 10

Consider the reaction below: F₂(g) → 2F(g) (a)Compressing the reaction mixture results in a change in Q.True or false? (b)Heating the reaction mixture causes the reaction to shift to the left.True or false? (c)At 1000 K,the equilibrium constant for the reaction is about 10^-4.If the reaction is perturbed such that Q = 1,the reaction must shift to the left.

Accepted Answer

The answer of Consider the reaction below: F₂(g) → 2F(g) (a)Compressing the...

Question 11

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g)concentration?

Accepted Answer

According to Le Chatelier's principle, when a system at equilibrium is subjected to a disturbance, it will respond in a way that counteracts the disturbance. In this case, increasing the temperature will shift the equilibrium in the endothermic direction to absorb the excess heat, leading to an increase in the concentration of NO₂. Therefore, the correct choice is E.

Question 12

The vapor pressure of acetic acid at 25S1U1P1$\circ$S1S1P0C is 16 Torr.$\Delta$G_r for the reaction CH₃COOH(l) →CH₃COOH(g) At 25S1U1P1$\circ$S1S1P0C is

Accepted Answer

At equilibrium, the Gibbs free energy change ($\Delta G_r$) for the phase transition from liquid to gas is zero.

Question 13

For any reaction at equilibrium,$\Delta$G < 0.

Accepted Answer

At equilibrium, $\Delta G = 0$, because there is no net change in the system's free energy.

Question 14

Consider the reaction 2HI(g) →H₂(g)+ I₂(g) At 298 K,K_c = 1.3 *10^-3,whereas at 783 K,K_c = 2.2 * 10^-2.Which of the following is true?

Accepted Answer

At a higher temperature of 783 K, the value of Kc increased from 1.3x10^10 to 2.2x10^10. This means that the product side (HSB and I2) is favored at higher temperatures. Therefore, the reaction is endothermic as it absorbs heat to form products. Additionally, we cannot determine whether the reaction is spontaneous or not just by knowing the value of Kc.

Question 15

For a pure solid or liquid,the molar free energy always has its standard value.

Accepted Answer

For a pure solid or liquid, the molar free energy is only dependent on temperature and pressure, and not on the amount or size of the sample. Therefore, it will always have a standard value at a given temperature and pressure, leading to a constant molar free energy per mol of substance.

Question 16

From a plot of Gibbs free energy versus progress of reaction,the sign of $\Delta$G_r at any point along the curve is given by the slope of the curve.

Accepted Answer

The slope of the Gibbs free energy versus progress of reaction curve at any point gives the sign of $\Delta G$, indicating whether the process is spontaneous ($\Delta G < 0$) or non-spontaneous ($\Delta G > 0$) at that point.

Question 17

If a reaction mixture that is not at equilibrium contains more products than reactants,$\Delta$G > 0 for the forward reaction.

Accepted Answer

According to Le Chatelier's principle, if a reaction mixture contains more products than reactants, then the system will shift towards the reactants to reach equilibrium. This means that the forward reaction is not at equilibrium and F1F1F1S1F1F1F10G > 0 (positive) for the forward reaction.

Question 18

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction,$\Delta$HS1U1P1$\circ$S1S1P0 = 92.38 kJ.mol^-1.

Accepted Answer

The answer of For the decomposition of ammonia to nitrogen...

Question 19

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Accepted Answer

The reaction is endothermic, so increasing the temperature will shift the equilibrium to the right, increasing the equilibrium constant.

Question 20

Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g) At 30S1U1P1$\circ$S1S1P0C and P_CO = 1 atm,Ni reacts with CO(g)to form Ni(CO)₄(g).At 200S1U1P1$\circ$S1S1P0C,Ni(CO)₄(g)decomposes to Ni(s)and CO(g).This means

Accepted Answer

The answer of Consider the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g) At 30S1U1P1$\circ$S1S1P0C...

Quiz 11: Chemical Equilibria

Consider the reaction CO(g) + 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Consider the reaction 4NH₃(g) + 3O₂(g) →2N₂(g) + 6H₂O(g) ,K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Consider the reaction 4NH₃(g)+ 7O₂(g) →2N₂O₄(g)+ 6H₂O(g) If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

The equilibrium constant K for the dissociation of N₂O₄(g) to NO₂(g) is 1700 at 500 K.Predict its value at 300 K.For this reaction, $\Delta$ H^$\circ$ is 56.8 kJ.mol^-1.

Consider the reaction 4NH₃(g) + 3O₂(g) →2N₂(g) + 6H₂O(g) ,K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g) concentration?

The vapor pressure of acetic acid at 25^$\circ$C is 16 Torr. $\Delta$ G_r for the reaction CH₃COOH(l) →CH₃COOH(g) At 25^$\circ$C is

For any reaction at equilibrium, $\Delta$ G < 0.

Consider the reaction 2HI(g) →H₂(g) + I₂(g) At 298 K,K_c = 1.3 10^-3,whereas at 783 K,K_c = 2.2 10^-2.Which of the following is true?

For a pure solid or liquid,the molar free energy always has its standard value.

From a plot of Gibbs free energy versus progress of reaction,the sign of $\Delta$ G_r at any point along the curve is given by the slope of the curve.

If a reaction mixture that is not at equilibrium contains more products than reactants, $\Delta$ G > 0 for the forward reaction.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction Ni(s) + 4CO(g) →Ni(CO) ₄(g) At 30^$\circ$C and P_CO = 1 atm,Ni reacts with CO(g) to form Ni(CO) ₄(g) .At 200^$\circ$C,Ni(CO) ₄(g) decomposes to Ni(s) and CO(g) .This means

Quiz 11: Chemical Equilibria

Consider the reaction CO(g) + 2H2(g) →CH3OH(g) At room temperature,K is approximately 2 * 104,but at a higher temperature K is substantially smaller.Which of the following is true?

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, Δ\DeltaΔ H ∘\circ∘ = 92.38 kJ.mol-1.

For the reaction 2NOCl(g) → 2NO(g)+ Cl2(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Consider the reaction 4NH3(g) + 3O2(g) →2N2(g) + 6H2O(g) ,K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

For the reaction 2NOCl(g) → 2NO(g)+ Cl2(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl2(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Consider the reaction 4NH3(g)+ 7O2(g) →2N2O4(g)+ 6H2O(g) If,initially,[NH3(g)] = [O2(g)] = 3.60 M,at equilibrium,[N2O4(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

The equilibrium constant K for the dissociation of N2O4(g) to NO2(g) is 1700 at 500 K.Predict its value at 300 K.For this reaction, Δ\DeltaΔ H ∘\circ∘ is 56.8 kJ.mol-1.

Consider the reaction 4NH3(g) + 3O2(g) →2N2(g) + 6H2O(g) ,K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)4(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)4(g) → Ni(s)+ 4CO(g)

For the reaction N2O4(g) →2NO2(g) Which of the following disturbances will cause an increase in NO2(g) concentration?

The vapor pressure of acetic acid at 25 ∘\circ∘ C is 16 Torr. Δ\DeltaΔ Gr for the reaction CH3COOH(l) →CH3COOH(g) At 25 ∘\circ∘ C is

For any reaction at equilibrium, Δ\DeltaΔ G < 0.

Consider the reaction 2HI(g) →H2(g) + I2(g) At 298 K,Kc = 1.3 *10-3,whereas at 783 K,Kc = 2.2 * 10-2.Which of the following is true?

For a pure solid or liquid,the molar free energy always has its standard value.

From a plot of Gibbs free energy versus progress of reaction,the sign of Δ\DeltaΔ Gr at any point along the curve is given by the slope of the curve.

If a reaction mixture that is not at equilibrium contains more products than reactants, Δ\DeltaΔ G > 0 for the forward reaction.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10-6 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction, Δ\DeltaΔ H ∘\circ∘ = 92.38 kJ.mol-1.

Consider the following N2O4(g) →2NO2(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction Ni(s) + 4CO(g) →Ni(CO) 4(g) At 30 ∘\circ∘ C and PCO = 1 atm,Ni reacts with CO(g) to form Ni(CO) 4(g) .At 200 ∘\circ∘ C,Ni(CO) 4(g) decomposes to Ni(s) and CO(g) .This means

Consider the reaction CO(g) + 2H₂(g) →CH₃OH(g) At room temperature,K is approximately 2 * 10⁴,but at a higher temperature K is substantially smaller.Which of the following is true?

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 1.00.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),if,initially,[NOCl(g)] = 2.8 M,at equilibrium [NO(g)] = 1.2 M.Calculate the equilibrium concentration of NOCl(g).

Consider the reaction 4NH₃(g) + 3O₂(g) →2N₂(g) + 6H₂O(g) ,K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of ammonia is

For the reaction 2NOCl(g) → 2NO(g)+ Cl₂(g),K = 98 at a certain temperature.If the equilibrium concentrations in a 1 L container are [NOCl(g)] = 1.0 M,[NO(g)] = 3.5 M and [Cl₂(g)] = 8.0 M,and 2.0 mol of each gas is added,in which direction does the reaction shift?

Consider the reaction 4NH₃(g)+ 7O₂(g) →2N₂O₄(g)+ 6H₂O(g) If,initially,[NH₃(g)] = [O₂(g)] = 3.60 M,at equilibrium,[N₂O₄(g)] = 0.60 M.Calculate the equilibrium concentrations of all other species.

The equilibrium constant K for the dissociation of N₂O₄(g) to NO₂(g) is 1700 at 500 K.Predict its value at 300 K.For this reaction, $\Delta$ H^$\circ$ is 56.8 kJ.mol^-1.

Consider the reaction 4NH₃(g) + 3O₂(g) →2N₂(g) + 6H₂O(g) ,K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

If the equilibrium constant for the reaction Ni(s)+ 4CO(g) →Ni(CO)₄(g)is 2.72 at a certain temperature,what is the equilibrium constant for the following reaction at the same temperature? Ni(CO)₄(g) → Ni(s)+ 4CO(g)

For the reaction N₂O₄(g) →2NO₂(g) Which of the following disturbances will cause an increase in NO₂(g) concentration?

The vapor pressure of acetic acid at 25^$\circ$C is 16 Torr. $\Delta$ G_r for the reaction CH₃COOH(l) →CH₃COOH(g) At 25^$\circ$C is

For any reaction at equilibrium, $\Delta$ G < 0.

Consider the reaction 2HI(g) →H₂(g) + I₂(g) At 298 K,K_c = 1.3 10^-3,whereas at 783 K,K_c = 2.2 10^-2.Which of the following is true?

From a plot of Gibbs free energy versus progress of reaction,the sign of $\Delta$ G_r at any point along the curve is given by the slope of the curve.

If a reaction mixture that is not at equilibrium contains more products than reactants, $\Delta$ G > 0 for the forward reaction.

For the decomposition of ammonia to nitrogen and hydrogen,the equilibrium constant is 1.47 * 10^-6 at 298 K.Calculate the temperature at which K = 0.0100.For this reaction, $\Delta$ H^$\circ$ = 92.38 kJ.mol^-1.

Consider the following N₂O₄(g) →2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Consider the reaction Ni(s) + 4CO(g) →Ni(CO) ₄(g) At 30^$\circ$C and P_CO = 1 atm,Ni reacts with CO(g) to form Ni(CO) ₄(g) .At 200^$\circ$C,Ni(CO) ₄(g) decomposes to Ni(s) and CO(g) .This means