Consider the following reaction:

2HF(g) H_{2}(g) + F_{2}(g) (K_{c} = 1.00 x 10^{–2})

Given that 1.00 mol of HF(g), 0.371 mol of H_{2}(g), and 0.750 mol of F_{2}(g) are mixed in a 5.00-L flask, determine the reaction quotient, Q.

d. Q = 2.12

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[HF(g)] = 1/5 = 0.2M

[H_{2}(g)] = 0.371/5 = 0.0742 M

[F_{2}(g)] = 0.750/5 =0.150 M

This reaction quotient = 0.0742*0.150/(0.2*0.2) = 0.278

Hence correct answer is (b)

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