1
Question
The manufacturing of ammonia by Haber's process involves the reaction with ΔH=−22.4kcal. When temperature is increased, the equilibrium is:
The manufacturing of ammonia by Haber's process involves the reaction with ΔH=−22.4kcal. When temperature is increased, the equilibrium is:
Open in App
Solution
The correct option is B shifted to the left
The negative value of the enthalpy of the reaction indicates that the formation of NH3 is an exothermic process.
When the temperature is increased, the reaction will proceed in the backward direction so as to absorb heat and nullify the effect of increasing temperature. In other words, the equilibrium will shift to left.
The negative value of the enthalpy of the reaction indicates that the formation of NH3 is an exothermic process.
When the temperature is increased, the reaction will proceed in the backward direction so as to absorb heat and nullify the effect of increasing temperature. In other words, the equilibrium will shift to left.
Suggest Corrections
0
Similar questions
View More
Join BYJU'S Learning Program
Explore more
Join BYJU'S Learning Program
