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

**The formula for Q is:**

$\overline{){\mathbf{Q}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

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

Consider the following reaction:

2HF_{ }_{(g)} ⇌ H_{2 }_{(g)} + F_{2(}_{g) }(Kc = 1.00 × 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.

A) Q = 0.0696

B) Q = 0.278

C) Q = 0.0557

D) Q = 2.12

E) none of these