a) the concentration of HI will rise as the system approaches equilibrium b) the

Question

a) the concentration of HI will rise as the system approaches equilibrium

b) the concentrations of HI and I2 will increase as the system approaches equilibrium

c) the concentration of H2 and I2 will increase as the system approaches equilibrium

EXPLAIN YOUR ANSWER

14) For the reaction, H2 (g) + I2 (g) 2HI (g), Kc= 50.2 at 445oC. If [H2] = [I2] = [HI] = 1.75*10-3 M at 445oC, which one of the following statements is true? [hint: what is Q?] a) the concentration of HI will rise as the system approaches equilibrium b) the concentrations of HI and I2 will increase as the system approaches equilibrium c) the concentration of H2 and I2 will increase as the system approaches equilibrium EXPLAIN YOUR ANSWER

Explanation / Answer

H2 + I2 -----------> 2HI

Q = [HI]2/[H2][I2]

Q = [1.75E-3]2/[1.75E-3][1.75E-3] = 0

If Q=0, then Q is less than K. Therefore, when Q=0, the reaction shifts to the right (forward). An easy way to remember this relationship is by thinking, “once you have nothing, the only thing left to do is to move forward.” If Q equals to zero, the reaction will shift forward (to the right).

So , the products will be favoured.

So, the true statement is a) the concentration of HI will rise as the system approaches equilibrium

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