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1 mole of H2O and 1 mole of CO are ta...

1 mole of `H_2O ` and 1 mole of CO are taken in a 10 litre vassel and heated to 725 K.At equilibrium 40 per cent of water (by mass ) reacts with carbon monoxide according to the equation
` H_2O(g) +CO( g) hArr H_2 (g)+ CO_2 (g)`
Calculate the equilibrium constant for the reactions.

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AI Generated Solution

To solve the problem, we will follow these steps: ### Step 1: Write the balanced chemical equation The balanced chemical equation for the reaction is: \[ \text{H}_2\text{O}(g) + \text{CO}(g) \rightleftharpoons \text{H}_2(g) + \text{CO}_2(g) \] ### Step 2: Determine initial concentrations We have 1 mole of H₂O and 1 mole of CO in a 10-liter vessel. The initial concentrations can be calculated as follows: ...
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One mole of H_(2)O and one mole of CO are taken in a 10 litre vessel and heated to 725 K . At equilibrium, 40 per cent of water (by mass) reacts with carbon monoxide according to the equation, H_(2)O_((g))+CO_((g))hArrH_(2(g))+CO_(2(g)) Calculate the equilibrium constant for the reaction.

For the equilibrium H_(2) O (1) hArr H_(2) O (g) at 1 atm 298 K

Knowledge Check

  • 1 mole of NO 1 mole of O_(3) are taken in a 10 L vessel and heated. At equilibrium, 50% of NO (by mass) reacts with O_(3) according to the equation : NO_((g))+O_(3(g))hArrNO_(2(g))+O_(2(g)) . What will be the equilibrium constant for this reaction ?

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    B
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