Chemistry · Stoichiometry
Work through this past-paper style MCQ, then read the full explanation. Practice more chemistry questions on mMCQ with adaptive practice and topic analytics.
For the chemical reaction
N2(g) +3H2(g) ->2NH3(g), we can maximize the yield by
- A
By increasing temperature
- B
By decreasing pressure
- C
By increasing volume of reaction vessel
- D
By continous withdrawl of ammonia after intervals
Continual withdrawal of NH3 shifts the equilibrium to the right side to balance the effect of decreasing the amount of NH3 (Le Chatelier principle). Hence, option D is correct.
The reaction is exothermic, so by increasing the temperature, the reaction will move in reverse direction. As a result, the yeild will become less. The option is incorrect.
If we decrease the pressure, the reaction will lean toward the reverse direction. It will lessen the product, so the option is incorrect.
If we would increase the volume, the reaction will move in the backward direction, decreasing the yield. This option is incorrect.
Continual withdrawal of NH3 shifts the equilibrium to the right side to balance the effect of decreasing the amount of NH3 (Le Chatelier principle). Hence, this option is correct.
Tagged under Chemistry · Stoichiometry · 2022