NEET2026ChemistryChapterActual
For the reaction CO(g) + H ₂ O(g) CO ₂ (g) + H ₂ (g) , the equilibrium constant K_c is 4.0 at a specific temperature. If a reaction mixture contains 0.1 M of CO , 0.1 M of H ₂ O , 0.4 M of CO ₂ , and 0.4 M of H ₂ at a given instant, predict the behavior of the system.
Options
- AThe reaction will proceed in the forward direction, consuming CO and H ₂ O .
- BThe reaction will proceed in the reverse direction, consuming CO ₂ and H ₂ .
- CThe equilibrium constant K_c will decrease to match the reaction quotient.
- DThe system is already at equilibrium, so no net change will occur.
Correct answer
B. The reaction will proceed in the reverse direction, consuming CO ₂ and H ₂ .
Step-by-step solution
The reaction quotient Q_c is calculated using the given concentrations of the species at the given instant: Q_c = [ CO ₂][ H ₂] [ CO ][ H ₂ O ] Substituting the given values: Q_c = 0.4 0.4 0.1 0.1 = 0.16 0.01 = 16 The equilibrium constant is given as K_c = 4.0 . Comparing Q_c and K_c , we find that Q_c > K_c . Since the reaction quotient is greater than the equilibrium constant, the system is not at equilibrium. To reach equilibrium, the reaction will proceed in the reverse direction, consuming the products CO ₂ an