Question 1

Consider the following reaction at equilibrium. What effect will adding more H₂S have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Accepted Answer

Adding more reactant (HS) to a system at equilibrium will shift the reaction to the right, towards the products, according to Le Chatelier's principle. This is because the system seeks to counteract the change and re-establish equilibrium.

Question 2

Consider the following reaction at equilibrium. What effect will adding He gas have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Accepted Answer

He gas is inert and does not participate in the reaction, therefore it will have no effect on the equilibrium position or equilibrium constant.

Question 3

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO₂(g) + 2H₂O(l) ⇌ CH₄(g) + 2O₂(g) Δ_rH° = +890 kJ

Accepted Answer

According to Le Chatelier's principle, a decrease in temperature favors the endothermic reaction which is the reaction in the forward direction. Therefore, the equilibrium will shift in the direction of reactants.

Question 4

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Accepted Answer

Since Ar is an inert gas and not involved in the reaction, adding it will not affect the equilibrium position or the equilibrium constant of the reaction. Therefore, no effect will be observed.

Question 5

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe₃O₄(s) + CO(g) ⇌ 3FeO(s) + CO₂(g) Δ_rH°= +35.9 kJ

Accepted Answer

According to Le Chatelier's principle, increasing the temperature of an exothermic reaction will cause the equilibrium to shift in the direction of the products to consume the excess heat. In this case, the reaction is exothermic because the enthalpy change is positive. Thus, increasing the temperature will shift the equilibrium in the direction of the products, resulting in an increase in the concentration of COS and FeO.

Question 6

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Accepted Answer

Le Chatelier's principle states that if a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress. Increasing the pressure of the reaction mixture will shift the equilibrium in the direction of the side with fewer moles of gas, which is the product side.

Question 7

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 8

Consider the following reaction at equilibrium. What effect will adding a catalyst have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Accepted Answer

Adding a catalyst does not affect the position of equilibrium or the equilibrium constant. It only speeds up the rate of both the forward and the reverse reactions equally, allowing the system to reach equilibrium faster but not affecting the equilibrium state itself.

Question 9

Consider the following reaction at equilibrium. What effect will removing H₂O have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 10

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 11

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Accepted Answer

According to Le Chatelier's Principle, when the volume of a reaction mixture is decreased, the system will try to counteract the change by shifting in the direction that produces fewer gas molecules. In this reaction, the products XeF₄(g) has one gas molecule and the reactants Xe(g) and 2F₂(g) have three gas molecules. Thus, the system will shift to the right in the direction of products to decrease the number of gas molecules and relieve the pressure.

Question 12

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Accepted Answer

Reducing the pressure of the reaction mixture will cause the equilibrium to shift towards the side with more moles of gas to counteract the change. In this reaction, the reactants side has 3 moles of gas (1 Xe + 2 F2) compared to 1 mole of gas on the products side (XeF4), so the reaction will shift towards the reactants.

Question 13

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 14

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C₃H₈(g) + 5O₂(g) ⇌ 3CO₂(g) + 4H₂O(l) Δ_rH° = -2220 kJ

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 15

Consider the following reaction at equilibrium. What effect will adding KCl have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Accepted Answer

Adding KCl will have no effect on the equilibrium because it is a solid and does not appear in the equilibrium expression.

Question 16

Consider the following reaction at equilibrium. What effect will removing NO₂ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Accepted Answer

Removing one of the reactant (NO₂) will cause a decrease in its concentration which according to Le Chatelier's principle, will shift the reaction to the side with more reactants in order to compensate for the loss. Therefore, the reaction will shift towards the reactants and the concentration of SO₂ and NO₂ will increase.

Question 17

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Accepted Answer

The answer of Consider the following reaction at equilibrium. What...

Question 18

Consider the following reaction at equilibrium. What effect will adding more SO₃ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Accepted Answer

Adding more SO₃ will shift the reaction towards the reactants according to Le Chatelier's principle, as the system seeks to counteract the change and re-establish equilibrium.

Question 19

For the reaction: N₂(g) + 2O₂(g) ⇌ 2NO₂(g), K_c = 8.3 × 10^-10 M^-1at 25 °C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Accepted Answer

The answer of For the reaction: N₂(g) + 2O₂(g) ⇌...

Question 20

Consider the following reaction at equilibrium. What effect will adding CO₂ have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

Accepted Answer

Adding CO₂ will increase the concentration of a reactant, causing the system to shift towards the products to re-establish equilibrium according to Le Chatelier's principle.

Quiz 14: Chemical Equilibrium

Consider the following reaction at equilibrium. What effect will adding more H₂S have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will adding He gas have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO₂(g) + 2H₂O(l) ⇌ CH₄(g) + 2O₂(g) Δ_rH° = +890 kJ

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe₃O₄(s) + CO(g) ⇌ 3FeO(s) + CO₂(g) Δ_rH°= +35.9 kJ

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will adding a catalyst have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will removing H₂O have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C₃H₈(g) + 5O₂(g) ⇌ 3CO₂(g) + 4H₂O(l) Δ_rH° = -2220 kJ

Consider the following reaction at equilibrium. What effect will adding KCl have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will removing NO₂ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Consider the following reaction at equilibrium. What effect will adding more SO₃ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

For the reaction: N₂(g) + 2O₂(g) ⇌ 2NO₂(g) , K_c = 8.3 × 10^-10 M^-1at 25 °C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Consider the following reaction at equilibrium. What effect will adding CO₂ have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

Quiz 14: Chemical Equilibrium

Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Consider the following reaction at equilibrium. What effect will adding He gas have on the system? 2KClO3(s) ⇌ 2KCl(s) + 3O2(g)

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO2(g) + 2H2O(l) ⇌ CH4(g) + 2O2(g) ΔrH° = +890 kJ

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe3O4(s) + CO(g) ⇌ 3FeO(s) + CO2(g) ΔrH°= +35.9 kJ

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Consider the following reaction at equilibrium. What effect will adding a catalyst have on the system? 2KClO3(s) ⇌ 2KCl(s) + 3O2(g)

Consider the following reaction at equilibrium. What effect will removing H2O have on the system? 2H2S(g) + 3O2(g) ⇌ 2H2O(g) + 2SO2(g)

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2F2(g) ⇌ XeF4(g)

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2F2(g) ⇌ XeF4(g)

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO2(g) + C(graphite) ⇌ 2CO(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5O2(g) ⇌ 3CO2(g) + 4H2O(l) ΔrH° = -2220 kJ

Consider the following reaction at equilibrium. What effect will adding KCl have on the system? 2KClO3(s) ⇌ 2KCl(s) + 3O2(g)

Consider the following reaction at equilibrium. What effect will removing NO2 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? CuS(s) + O2(g) ⇌ Cu(s) + SO2(g)

Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

For the reaction: N2(g) + 2O2(g) ⇌ 2NO2(g) , Kc = 8.3 × 10-10 M-1 at 25 °C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?

Consider the following reaction at equilibrium. What effect will adding CO2 have on the system? CO2(g) + C(graphite) ⇌ 2CO(g)

Consider the following reaction at equilibrium. What effect will adding more H₂S have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will adding He gas have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will decreasing the temperature have on the system? CO₂(g) + 2H₂O(l) ⇌ CH₄(g) + 2O₂(g) Δ_rH° = +890 kJ

Consider the following reaction at equilibrium. What effect will adding 1 mole of Ar to the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? Fe₃O₄(s) + CO(g) ⇌ 3FeO(s) + CO₂(g) Δ_rH°= +35.9 kJ

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will adding a catalyst have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will removing H₂O have on the system? 2H₂S(g) + 3O₂(g) ⇌ 2H₂O(g) + 2SO₂(g)

Consider the following reaction at equilibrium. What effect will increasing the pressure of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Consider the following reaction at equilibrium. What effect will reducing the pressure of the reaction mixture have on the system? Xe(g) + 2F₂(g) ⇌ XeF₄(g)

Consider the following reaction at equilibrium. What effect will adding some C have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)

Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C₃H₈(g) + 5O₂(g) ⇌ 3CO₂(g) + 4H₂O(l) Δ_rH° = -2220 kJ

Consider the following reaction at equilibrium. What effect will adding KCl have on the system? 2KClO₃(s) ⇌ 2KCl(s) + 3O₂(g)

Consider the following reaction at equilibrium. What effect will removing NO₂ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

Consider the following reaction at equilibrium. What effect will reducing the volume of the reaction mixture have on the system? CuS(s) + O₂(g) ⇌ Cu(s) + SO₂(g)

Consider the following reaction at equilibrium. What effect will adding more SO₃ have on the system? SO₂(g) + NO₂(g) ⇌ SO₃(g) + NO(g)

For the reaction: N₂(g) + 2O₂(g) ⇌ 2NO₂(g) , K_c = 8.3 × 10^-10 M^-1at 25 °C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is five times the concentration of O₂ gas?

Consider the following reaction at equilibrium. What effect will adding CO₂ have on the system? CO₂(g) + C(graphite) ⇌ 2CO(g)