For H2(g) + I2(g) 2HI(g), K_c = 50 at a certain temperature. A 5.0 L flask contains 0.50 mol H2, 0.50 mol I2 and 3.00 mol HI. Which statement is correct?

Q_c = 36, so the net reaction is forward

Q_c = 36, so the net reaction is backward

Q_c = 60, so the net reaction is backward

Q_c = 0.028, so the net reaction is forward

Q_c = 36, so the net reaction is forward

JEE Main levelSingle correct optionDifficulty 2 of 3ce015

For $H X_{2} (g) + I X_{2} (g) 2 HI (g)$ , $K_{c} = 50$ at a certain temperature. A 5.0 L flask contains 0.50 mol $H X_{2}$ , 0.50 mol $I X_{2}$ and 3.00 mol $HI$ . Which statement is correct?

Since

Δ n_{g} = 0

, the volume cancels:

Q_{c} = (3.00)^{2} / ((0.50) (0.50)) = 36

(using mol directly). As

Q_{c} < K_{c} = 50

, the mixture shifts forward, forming more

HI