Multiple Choice
Consider the following equilibrium, for which Kp = 7.54×10⁻² at 490 °C: 2Cl2(g) + 2H2O(g) ⇌ 4HCl(g) + O2(g). What is the value of Kc for the following reaction? Cl2(g) + H2O(g) ⇌ 2HCl(g) + 0.5O2(g)
16. Chemical Equilibrium
Equilibrium Constant K
Multiple Choice
For the combustion reaction 2H₂(g) + O₂(g) → 2H₂O(g), what is the likely magnitude of the equilibrium constant K at a given temperature?
A
K ≈ 1
B
K >> 1
C
K << 1
D
K = 0
Verified step by step guidance1
Identify the type of reaction: The given reaction is a combustion reaction where hydrogen gas (H₂) reacts with oxygen gas (O₂) to form water vapor (H₂O). Combustion reactions are typically exothermic, releasing energy.
Understand the equilibrium constant (K): The equilibrium constant, K, is a measure of the extent of a reaction at equilibrium. It is defined as the ratio of the concentration of products to the concentration of reactants, each raised to the power of their stoichiometric coefficients.
Write the expression for the equilibrium constant (K): For the reaction 2H₂(g) + O₂(g) → 2H₂O(g), the equilibrium constant expression is K = \( \frac{[H_2O]^2}{[H_2]^2[O_2]} \).
Analyze the reaction: Since the reaction is highly exothermic and proceeds almost completely to form water, the concentration of products (H₂O) at equilibrium is much higher than the concentration of reactants (H₂ and O₂).
Conclude the magnitude of K: Given that the reaction proceeds almost to completion, the equilibrium constant K is expected to be much greater than 1 (K >> 1), indicating a product-favored reaction at equilibrium.
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