Problem: Consider the following reaction:2HF (g) ⇌ H2 (g) + F2(g) (Kc = 1.00 × 10–2)Given that 1.00 mol of HF(g), 0.371 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q.A) Q = 0.0696B) Q = 0.278C) Q = 0.0557D) Q = 2.12E) none of these

FREE Expert Solution

We are being asked to calculate the reaction quotient, Q:


The formula for Q is:


Q = productsreactants


Depending on if Q is greater than or less than K our reaction will shift to attain equilibrium by reaching the equilibrium constant K:


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Problem Details

Consider the following reaction:

2HF (g) ⇌ H(g) + F2(g) (Kc = 1.00 × 10–2)

Given that 1.00 mol of HF(g), 0.371 mol of H2(g), and 0.750 mol of F2(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q.

A) Q = 0.0696

B) Q = 0.278

C) Q = 0.0557

D) Q = 2.12

E) none of these