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Standard XII

Chemistry

Le Chatelier's Principle for Del N Equals to 0

An industrial...

Question

An industrial fuel, 'water gas', which consists of a mixture of $H_{2}$ and CO can be made by passing steam over
red hot carbon. The reaction is :
$C (s) + H_{2} O ⇌ C O (g) + H_{2} O, Δ H = + 131 k J$
The yield of CO and $H_{2}$ at equilibrium would be shifted to the product side by :

raising the realtive pressure of the steam

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adding hot carbon

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raising the temperature

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reducing the volume of the system

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Solution

The correct options are
B raising the realtive pressure of the steam
C raising the temperature
For the reaction,
$C (s) + H_{2} O ⇌ C O (g) + H_{2} (g)$ , $Δ H$ is positive.
Hence, it is an endothermic reaction. So, on increasing the temperature, there is excess heat present in the reaction. This heat can be absorbed in an endothermic reaction, which is the forward reaction.
Also, if partial pressure of steam on the reactant side is raised, then the reaction constant will be less than the equilibrium constant. Hence, the reaction will move in forward reaction, so as to decrease the relative pressure of steam and increase the reaction constant to make it equal to equilibrium constant.

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Similar questions

Q. An industrial fuel, 'water gas', which consists of a mixture of

H_{2}

and

C O

can be made by passing steam over red-hot carbon. The reaction is:

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g), Δ H = + 131 k J

The yield of the product can be increased by:

Q. Water gas, an individual fuel, consisting

C O

and

H_{2}

in equimolar amounts is obtained by passing steam over red-hot carbon in accordance with the reaction:

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g); Δ H = + 130.5 k J

The yield of water gas can be increased by:
(1) Reducing the total pressure of the system
(2) Increasing pressure of steam
(3) Raising the temperature
(4) Introducing hot carbon

Q. Water gas, a mixture of

H_{2}

and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. Write the expression for the equilibrium for the equilibrium constant for the reversible reaction.

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g)

Δ H = 131.30

kJ.

Q. Water gas, a mixture of

H_{2}

and

C O

, is an important industrial fuel produced by the reaction of steam with red-hot coke,essentially pure carbon. Write the expression for the equilibrium constant for the reversible reaction.

C (s) + H_{2} O (g) ⇌ C O (g) + H_{2} (g) Δ H = 131.30 k J

Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high temperature steam. The first stage of two stage reaction involves the formation of CO and H₂. In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction,

If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam such that 4.0 bar, what will be the partial pressure of H₂ at equilibrium? Kp= 10.1 at 400°C

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An industrial fuel, 'water gas', which consists of a mixture of H2 and CO can be made by passing steam over red hot carbon. The reaction is :C(s)+H2O⇌CO(g)+H2O,ΔH=+131kJThe yield of CO and H2 at equilibrium would be shifted to the product side by :

An industrial fuel, 'water gas', which consists of a mixture of $H_{2}$ and CO can be made by passing steam over
red hot carbon. The reaction is :
$C (s) + H_{2} O ⇌ C O (g) + H_{2} O, Δ H = + 131 k J$
The yield of CO and $H_{2}$ at equilibrium would be shifted to the product side by :