in haber process 30 litres of di hydrogen and 30 litres of di nitrogen were taken for reaction wch yielded only 50% of the expected product. what will be the composition of the gaseous mixture under the aforesaid condition in the end
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Haber's process is industrial or commercial process used for the manufacture of ammonia from nitrogen and hydrogen using iron catalyst at 400-450 degree Celsius and 200 atmospheres pressure.
A mixture of hydrogen and nitrogen gases in the ratio 3:1 is taken in compressor. It is then compressed to about 200 atm pressure and passed over heated catalyst in catalyst chamber. The mixture is maintained at a temperature between 400 − 450°C. In condenser, the hot mixture of ammonia gas and unreacted hydrogen and nitrogen gases coming out of catalyst chamber are led to cooling pipes.
The reaction is reversible and exothermic in nature.
Catalysts such as iron oxide with small amounts of molybdenum are used to increase the rate of attainment of equilibrium.
High pressure favours the formation of NH 3 .
Optimum condition : Pressure = 200 × 10 5 Pa (about 200 atm)
Temperature ∼ 700 K
The unused mixture of hydrogen and nitrogen gases are recompressed and then recycled into catalyst chamber.
(ii) For the haber process, reaction is :
N2 (g) +3 H2(g) →2 NH3
According to the Gay Lussac law , 1 L of the N2 gas would react with 3 L of H2 gas to produce 2 L of NH3.
Since 30 L of N2 and 30 L of H2 gas are present thus according to the balanced equation H2 is the limiting reagent .
Thus 30 L H2 gas on reaction with 10 L N2should produce 20 L NH3. But since it is given that only 50% of the expected product is obtained . This shows that only 15 L of H2 gas is reacting with 5 L N2 gas to give half of the expected product i.e. 10 LNH3 gas.
Thus composition of gases in the reaction mixture :
Amount of N2 gas left in the reaction vessel = 30-5 = 25 L
Amount of H2 gas left in the reaction vessel = 30-15 = 15 L
Amount of NH3 gas produced in the reaction vessel = 10 L
A mixture of hydrogen and nitrogen gases in the ratio 3:1 is taken in compressor. It is then compressed to about 200 atm pressure and passed over heated catalyst in catalyst chamber. The mixture is maintained at a temperature between 400 − 450°C. In condenser, the hot mixture of ammonia gas and unreacted hydrogen and nitrogen gases coming out of catalyst chamber are led to cooling pipes.
The reaction is reversible and exothermic in nature.
Catalysts such as iron oxide with small amounts of molybdenum are used to increase the rate of attainment of equilibrium.
High pressure favours the formation of NH 3 .
Optimum condition : Pressure = 200 × 10 5 Pa (about 200 atm)
Temperature ∼ 700 K
The unused mixture of hydrogen and nitrogen gases are recompressed and then recycled into catalyst chamber.
(ii) For the haber process, reaction is :
N2 (g) +3 H2(g) →2 NH3
According to the Gay Lussac law , 1 L of the N2 gas would react with 3 L of H2 gas to produce 2 L of NH3.
Since 30 L of N2 and 30 L of H2 gas are present thus according to the balanced equation H2 is the limiting reagent .
Thus 30 L H2 gas on reaction with 10 L N2should produce 20 L NH3. But since it is given that only 50% of the expected product is obtained . This shows that only 15 L of H2 gas is reacting with 5 L N2 gas to give half of the expected product i.e. 10 LNH3 gas.
Thus composition of gases in the reaction mixture :
Amount of N2 gas left in the reaction vessel = 30-5 = 25 L
Amount of H2 gas left in the reaction vessel = 30-15 = 15 L
Amount of NH3 gas produced in the reaction vessel = 10 L
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