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Commercially, ammonia (NH(3)) is produce...

Commercially, ammonia `(NH_(3))` is produced from nitrogen `(N_(2))` and hydrogen `(H_(2))` using the Haber process
`N_(2)(g) + 3H_(2) ( g) rarr 2NH_(3)(g)`
This reaction is exothermic. Which of the following would increase the amount of `NH_(3)` obtained (i.e. maximize the yield of `NH_(3)`) at equilibrium ?
(i) Decrease the pressure (ii) Increase the temperature
(iii) Increase the concentration of `N_(2)` (iv) Increase the concentration of `NH_(3)`
( v ) Decrease the concentration of `H_(2)`

A

I,II,IV and V

B

I and III

C

II and III

D

III only

Text Solution

Verified by Experts

The correct Answer is:
D
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Knowledge Check

  • For the reaction N_(2)(g) + 3H_(2)(g) rarr 2NH_(2)(g) Which of the following is correct?

    A
    `DeltaH = DeltaU`
    B
    `DeltaH gt DeltaU`
    C
    `DeltaH lt DeltaU`
    D
    `DeltaH = 2 DeltaU`

  • N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) + heat .What is the effect of the increase of temperature on the equilibrium of the reaction ?

    A
    Equilibrium is shifted to the left
    B
    Equilibrium is shifted to the right
    C
    Equilibrium is unaltered
    D
    Reactions rate does not change

  • In the manufacture of ammonia by Haber's process, N_(2)(g) +3H_(2)(g) hArr 2NH_(3)(g)+92.3kJ , which of the following conditions is unfavourable ?

    A
    increasing the temperature
    B
    increasing the pressure
    C
    reducing the temperture
    D
    removing ammonia as it is formed.

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