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Water gas, an individual fuel, consisting \[\text{CO and }{{\text{H}}_{2}}\]in equimolar amounts is obtained by passing steam over red-hot carbon in accordance with the reaction:
\[{{\text{C}}_{\left( \text{s} \right)}}\text{ + }{{\text{H}}_{2}}\text{O }\rightleftharpoons \text{ C}{{\text{O}}_{\left( \text{g} \right)}}\text{ + }{{\text{H}}_{2\left( \text{g} \right)}};\Delta \text{H = +130}\text{.5kJ}\]
The yield of water gas can be increased by:
(1) Reducing the total pressure of the system
(2) Increasing pressure of atom
(3) Raising the temperature
(4) Introducing hot carbon
A. 1, 2 and 3 are correct
B. 1 and 2 are correct
C. 2 and 4 are correct
D. 1 and 3 are correct

Last updated date: 29th Feb 2024
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IVSAT 2024
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Hint: Every reaction has different conditions of temperature, pressure and nature of the reaction. According to the Le Chatelier principle, each response to the changes that are made in the reaction tries to gain equilibrium state again.

Complete Answer:
-For the given reaction, we know that the value of \[\Delta \text{H}\] is positive as given in the question.
-The value enthalpy change or \[\Delta \text{H}\] is positive, when the heat is absorbed in the reaction it means the reaction is endothermic.
-So, if we will increase the temperature of the reaction then it will favour the forward reaction.
-So, option 3 is the correct answer.
-If the pressure of the atom will be increased then the reaction constant will become less than the equilibrium constant.
-It will favour the reaction to move in a forward direction.
-So, option 2 is also the correct answer.
-If the total pressure of the system is reduced then it allows more moles of a water molecule to react.
-Hence, reducing the total pressure of the system will favour the forward reaction.
-So, option 1 is also the correct answer.

Therefore, option A. is the correct answer.

Note: The equilibrium constant tells us whether the product and reactant molecules are in the equilibrium state or not. If the change in enthalpy has a negative value then it indicates that the reaction is exothermic.
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