What would cause the equilibrium to shift left in this reaction? CO + 3H2 ⇌ CH4 + H2O

A) adding heat to the product mixture

B) a faster rate of forward reaction

C) increased collisions between CO and H2

D) the escape of water from the mixture

E) placing the mixture in a cold water bath

Explanation:

Option A. Explanation: To decrease pressure by increasing volume, the equilibrium of the reaction shift to the left as the reactant side has greater number of moles than the product side

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml