At a temperature of 700 K, the forward and reverse rate constants for the reaction 2 HI(g) ⇌ H₂(g) + I₂(g) are k_f = 1.8×10⁻³⁰ M⁻¹s⁻¹ and k_r = 0.063 M⁻¹s⁻¹.
(a) What is the value of the equilibrium constant K_c at 700 K?
(b) Is the forward reaction endothermic or exothermic if the rate constants for the same reaction have values of k_f= 0.097M⁻¹s⁻¹ and k_r= 2.6 M⁻¹s⁻¹ at 800 K?

검증된 단계별 안내

First, recall that the equilibrium constant (K) for a reaction is given by the ratio of the forward rate constant (kf) to the reverse rate constant (kr). So, K = kf/kr.

Calculate the equilibrium constant at 700 K using the given rate constants. K1 = kf1/kr1.

Next, calculate the equilibrium constant at 800 K using the given rate constants. K2 = kf2/kr2.

Compare the two equilibrium constants. If K2 > K1, the reaction shifts to the right (towards the products) as the temperature increases, indicating that the reaction is endothermic. If K2 < K1, the reaction shifts to the left (towards the reactants) as the temperature increases, indicating that the reaction is exothermic.

Remember, an endothermic reaction absorbs heat from its surroundings (ΔH > 0), while an exothermic reaction releases heat to its surroundings (ΔH < 0).

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Rate Constants and Temperature

Rate constants (k) are values that indicate the speed of a reaction at a given temperature. They are influenced by temperature changes, typically increasing with higher temperatures due to increased molecular energy and collision frequency. Understanding how rate constants vary with temperature is crucial for analyzing reaction kinetics and determining the nature of the reaction.

Equilibrium and Le Chatelier's Principle

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. Le Chatelier's Principle states that if a system at equilibrium is disturbed, it will shift in a direction that counteracts the disturbance. This principle helps predict how changes in temperature or concentration affect the position of equilibrium.

Endothermic vs. Exothermic Reactions

Endothermic reactions absorb heat from their surroundings, leading to a decrease in temperature, while exothermic reactions release heat, increasing the temperature. The nature of a reaction can be inferred from the temperature dependence of the rate constants; if increasing temperature increases the rate of the endothermic forward reaction more than the reverse, it suggests the forward reaction is endothermic.