Question 1

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g). Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?

Accepted Answer

Adding carbon monoxide (CO) to the system increases the concentration of one of the reactants. According to Le Chatelier's principle, the system will respond by shifting the equilibrium to the right to consume the added CO, thus producing more products until a new equilibrium is established.

Question 2

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g). Explain what would happen to the equilibrium upon the addition of hydrogen gas?

Accepted Answer

The addition of hydrogen gas increases the concentration of one of the products, causing the equilibrium to shift to the left to counteract this change, resulting in the formation of more reactants.

Question 3

If the reaction quotient is greater than the equilibrium constant, which statement would be correct?

Accepted Answer

When the reaction quotient (Q) is greater than the equilibrium constant (K), it indicates that there are more products relative to reactants than at equilibrium. Therefore, the reaction will shift towards the reactants (to the left) to reach equilibrium.

Question 4

Write the equilibrium expression for H₂Og) + COg) ⇌ H₂g) + CO₂g).

Accepted Answer

The equilibrium expression for a reaction is written as the product of the concentrations of the products raised to their stoichiometric coefficients, divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients. In this case, the correct expression is [COS][H2O]/[H2][CO], which matches choice A.

Question 5

The K_c for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I₂, and H₂ are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

Accepted Answer

The reaction quotient Q is calculated using the formula Q = [HI]^2 / ([I2] * [H2]), substituting the given concentrations gives Q = (0.338)^2 / (0.112 * 0.198) = 5.15. Since Q < Kc (54), the reaction will proceed to the right to reach equilibrium.

Question 6

Write the equilibrium expression for 2NOg) + 2H₂g) ⇌ N₂g) + 2H₂Og).

Accepted Answer

The equilibrium expression is written as the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients.

Question 7

If the reaction quotient is less than the equilibrium constant, which statement would be correct?

Accepted Answer

When the reaction quotient (Q) is less than the equilibrium constant (K), it indicates that there are not enough products relative to reactants. Therefore, the reaction will proceed in the forward direction (towards the right) to produce more products and reach equilibrium.

Quiz 13: Fundamental Equilibrium Concepts

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g) . Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g) . Explain what would happen to the equilibrium upon the addition of hydrogen gas?

If the reaction quotient is greater than the equilibrium constant, which statement would be correct?

Write the equilibrium expression for H₂Og) + COg) ⇌ H₂g) + CO₂g) .

The K_c for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I₂, and H₂ are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

Write the equilibrium expression for 2NOg) + 2H₂g) ⇌ N₂g) + 2H₂Og) .

If the reaction quotient is less than the equilibrium constant, which statement would be correct?

Quiz 13: Fundamental Equilibrium Concepts

Consider the following equilibrium mixture in a closed system: H2Og) + COg) ⇌ H2g) + CO2g) . Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?

Consider the following equilibrium mixture in a closed system: H2Og) + COg) ⇌ H2g) + CO2g) . Explain what would happen to the equilibrium upon the addition of hydrogen gas?

If the reaction quotient is greater than the equilibrium constant, which statement would be correct?

Write the equilibrium expression for H2Og) + COg) ⇌ H2g) + CO2g) .

The Kc for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I2, and H2 are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

Write the equilibrium expression for 2NOg) + 2H2g) ⇌ N2g) + 2H2Og) .

If the reaction quotient is less than the equilibrium constant, which statement would be correct?

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g) . Explain what would happen to the equilibrium upon the addition of carbon monoxide gas?

Consider the following equilibrium mixture in a closed system: H₂Og) + COg) ⇌ H₂g) + CO₂g) . Explain what would happen to the equilibrium upon the addition of hydrogen gas?

Write the equilibrium expression for H₂Og) + COg) ⇌ H₂g) + CO₂g) .

The K_c for the formation of HI from iodine and hydrogen gas is 54. If the concentrations of HI, I₂, and H₂ are 0.338 M, 0.112 M, and 0.198 M respectively, which statement is correct?

Write the equilibrium expression for 2NOg) + 2H₂g) ⇌ N₂g) + 2H₂Og) .