The equilibrium constant is 8.8 x 10^2 at a particular temperature for the react

Question

The equilibrium constant is 8.8 x 10^2 at a particular temperature for the reaction: H2(g) + I2(g) ? 2HI(g) Use this information to decide what will happen, given the following sets of initial conditions: Will the reaction shift to the left, to the right or will the system be at equilibrium? 1. PH2 = 0.5092 torr,PI2 = 0.079 torr, PHI = 5.95 torr 2. A 2.0 L flask contains 0.0591 mol H2, 0.009 mol I2 and 0.684 mol HI. 3. A 1.0 L flask contains 1.15 mol H2, 0.081 mol I2 and 8.35 mol HI. 4. PH2 = 0.35 torr, PI2 = 0.069 torr, PHI = 6.05 torr

Explanation / Answer

1) keq = (5.95)^2 / (0.5092 *0.079 ) = 8.8 * 10^2
hence the reaction will be at equilibruium
2) Keq = 0.6842 / (0.0591*0.009) = 8.79 * 10^2 therefore a mild shift to left side

3)K eq = 8.35 ^2 / (1.15 * 0.081) = 7.48 * 10^2 ; hence shift to left hand side

4) K eq = 6.05^2 /( 0.35 * 0.069) = 15.15 * 10^2 , shift to right side

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