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Haber Bosch Process

In the Haber ...

Question

In the Haber process for the industrial manufacturing of ammonia involving the reaction
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)$ at $200 a t m$ pressure in the presence of a catalyst, a temperature of about $500^{o} C$ is used. This is considered as optimum temperature for the process because:

yield is maximum at this temperature

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catalyst is active only at this temperature

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energy needed for the reaction is easily obtained at this temperature

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rate of the catalytic reaction is fast enough while the yield is also appreciable for this exothermic reaction at this temperature

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Solution

The correct option is A yield is maximum at this temperature
In order to yield the maximum yield of ammonia, the temperature is lowered though $500^{o} C$ is not a low temperature. This temperature $(500^{o} C)$ is a compromise temperature to produce reasonably a high proportion of ammonia in the equilibrium mixture in a very short time.

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Similar questions

Q. In the Haber process for the industrial manufacture of ammonia involving the reaction,

N_{2} + 3 H_{2} ⇌ 2 N H_{3}

at 200 atm pressure in the presence of a catalyst, a temperature of about 500

^{o}

C is used. This is considered as optimum temperature for the process because _______.

In Haber's process, the ammonia is manufactured according to the following reaction:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g); Δ H^{o} = - 22.4 k J / m o l

The pressure inside the chamber is maintained at

200

atm and temperature at

500^{o} C

. Generally, this reaction is carried out in the presence of

F e

catalyst.

500^{o} C

is considered optimum temperature for Haber's process because:

Q. At

450^{o} C

, the equilibrium constant

K_{p}

for the reaction,

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)

, was found to be

1.6 \times 10^{- 5}

at a pressure of

200 a t m

. If

N_{2}

and

H_{2}

are taken in

1 : 3

ratio, what is % of

{N H}_{3}

formed at this temperature?

Q. The equilibrium constant

K_{p}

for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)

1.64 \times 10^{- 4}

400^{o} C

and

0.144 \times 10^{- 4}

500^{o} C

. Calculate the mean heat of formation of

1

mole of

{N H}_{3}

from its elements in this temperature range.

Q. The reaction between

N_{2}

and

H_{2}

to form ammonia has

K_{C} = 6 \times 10^{- 2}

at the temperature

500^{o} C

. The numerical value of

K_{p}

for this reaction is;

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In the Haber process for the industrial manufacturing of ammonia involving the reactionN2(g)+3H2(g)⇌2NH3(g) at 200atm pressure in the presence of a catalyst, a temperature of about 500oC is used. This is considered as optimum temperature for the process because:

In the Haber process for the industrial manufacturing of ammonia involving the reaction
$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)$ at $200 a t m$ pressure in the presence of a catalyst, a temperature of about $500^{o} C$ is used. This is considered as optimum temperature for the process because: