Question

24. The reaction: H2 (g) + I2 (g) <--> 2 HI (g) has a Keq = 20.0 If the initial concentrations give a value less than 20, we can say:
a. the reaction will move to the reagents to reach equilibrium
b. by increasing the volume of the reaction container, the system will reach equilibrium
c. reducing the volume causes the reaction to reach equilibrium
d. the reaction will move towards the products to reach equilibrium

Answer 1

For the reaction H (git Iz (g) ? 2HIG) Given that keq = 20 Keq = [HI]" where, all the concentrations are 12] [[2] molar concentrations at equilibrium The ratio [Hif at any instant other than equilibrium H] [2] is known as reaction quotient Q. Given that Q 420, meas numerator is lesser than denomenator. This indicates that I < [[+ I) eam initial The system will try to attain equilibrium. or the reactions shifts from left to right ie towards product if & & Keg. Answer: d, the xxn will move to product side to reach equilibrium. Increasing volume, will decrease pressure and decreasing volume will increase pressure. But change in pressure has no effect on equilibrium for this reaction as number of moles of produt is equal to that of reactants. Ang = n - n = 0. b and c are not correct.