Question

The equilibrium constant is 8.8 x 102 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? A 4.0 L flask contains 1.17 mol H2, 0.083 mol I2 and 8.11 mol HI. A 2.0 L flask contains 0.0455 mol H2, 0.012 mol I2 and 0.693 mol HI. PH2 = 0.5380 torr,PI2 = 0.066 torr, PHI = 5.59 torr PH2 = 0.47 torr, PI2 = 0.061 torr, PHI = 5.99 torr

Answer 1

Answer:

when the balanced equation for the reaction is:

          H2(g) + i2(g)⇄ 2Hi

initial    0.5      0.5        X

            -X        -X         +X

Final (0.5-x)    (0.5-x)   2X

by substitution at the Kc formula:

Kc= [Hi]^2 / [H2] * [i2]

53.3 = (2X)^2 / (0.5-X) (0.5-X)by taking the square route

√53.3 = 2X / (0.5-X)

∴X = 0.39 m

∴[Hi] = 0.39 m