Question

A mixture of reactants and products has a equilibrium constant of 4.7 and initially contains 0.035 M H2O, 0.050 M CH4, 0.15 M CO, and 0.20 M H2. In which direction will the reaction go in order to attain equilibrium?

Answer 1

Answer: Reaction will move in forward direction in order to attain an equilibrium.

Step-by-step explanation:

• 
  `K_c>Q_c` reaction will move in forward direction.

• 
  `Q_c>K_c` reaction will move in backward direction.

• 
  `Q_c=K_c` reaction is at equilibrium.

`CH_4+H_2O\rightleftharpoons CO+3H_2`

`K_(c)=4.7`

`[H_2O]=0.035 M,[CH_4]=0.050 M,[CO]=0.15 M,[H_2]=0.20 M`

The expression for equilibrium quotient is written as :

`Q_(c)=([CO][H_2]^3)/([H_2O][CH_4])=(0.15* (0.20)^3)/(0.035* 0.050)=0.6857`

Since,
`K_c>Q_c` reaction will move in forward direction.