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.
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
For the reaction NH2COONH4(s) $\rightleftharpoons$2NH3(g) + CO2(g), KP = 3.2 × 10−5 atm3. The total pressure of the gase...The equilibrium constant for reaction H2(g) + CO2(g) ⇋ H2O(g) + CO(g) is 1·8 at 1000oC. If one mole of H2 and 1·0 ...For the reaction: CuSO4.3H2O(s) $\rightleftharpoons$CuSO4.H2O(s) + 2H2O(g); ΔH = 3360 cal. The dissociation pressure is ...At 1000oC and a pressure of 16 atm, the equilibrium constant of the reaction CO2(g) + C(s) $\rightleftharpoons$2CO(g) is...What is/are true about equilibrium state?...