Chemical EquilibriumHard
Question
In the Haber process for the industrial manufacturing of ammonia involving the reaction,
N2(g) + 3H2(g) ⇋ 2NH3(g) at 200 atm pressure in the presence of a catalyst, a temperature of about 500oC is used. This is considered as optimum temperature for the process because
N2(g) + 3H2(g) ⇋ 2NH3(g) at 200 atm pressure in the presence of a catalyst, a temperature of about 500oC is used. This is considered as optimum temperature for the process because
Options
A.yield is maximum at this temperature
B.catalyst is active only at this temperature
C.energy needed for the reaction is easily obtained at this temperature
D.rate of the catalytic reaction is fast enough while the yield is also appreciable for this exothermic reaction at this temperature.
Solution
On increasing temperature though reaction equilibrium shifts in the backward direction but for rate of reaction to be higher, higher temperature is required and particle 500oC is found to be optimum temperautre.
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