For the reaction CO2 (g) + H2(g) ↔ CO(g) + H2O(g) the value of K at 552°C is 0.137. If 3.0 moles of CO2, 3.0 moles of H2 , 1.5 mole of CO and 1.5 mole of H2O are initially present in a 1.0 L closed vessel, what are the actual concentrations of CO2, H2,CO and H2O at equilibrium

Question

Sakshi · Answer

For this reaction, as one can see that 1 mole of CO₂ react with one mole of H₂ to give one mole of CO and one mole of H₂0.
If one assumes that x mole of CO₂ gets used up in the reaction, the value of all the species at equilibrium will be CO₂(3-x), H₂( 3-x), CO (1.5 + x) and H₂O (1.5 + X)
Then, on using the value of equilibrium constant as
0.137= (1.5 + x) ²/ (3-x) ²
On solving and substituting the value of x, one can find the ans to the above question.
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For the reaction CO2 (g) + H2(g) ↔ CO(g) + H2O(g) the value of K at 552°C is 0.137. If 3.0 moles of CO2, 3.0 moles of H2 , 1.5 mole of CO and 1.5 mole of H2O are initially present in a 1.0 L closed vessel, what are the actual concentrations of CO2, H2,CO and H2O at equilibrium

For the reaction CO2 (g) + H2(g) ↔ CO(g) + H2O(g) the value of K at 552°C is 0.137. If 3.0 moles of CO2, 3.0 moles of H2 , 1.5 mole of CO and 1.5 mole of H2O are initially present in a 1.0 L closed vessel, what are the actual concentrations of CO2, H2,CO and H2O at equilibrium

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For the reaction CO2 (g) + H2(g) ↔ CO(g) + H2O(g) the value of K at 552°C is 0.137. If 3.0 moles of CO2, 3.0 moles of H2 , 1.5 mole of CO and 1.5 mole of H2O are initially present in a 1.0 L closed vessel, what are the actual concentrations of CO2, H2,CO and H2O at equilibrium

For the reaction CO2 (g) + H2(g) ↔ CO(g) + H2O(g) the value of K at 552°C is 0.137. If 3.0 moles of CO2, 3.0 moles of H2 , 1.5 mole of CO and 1.5 mole of H2O are initially present in a 1.0 L closed vessel, what are the actual concentrations of CO2, H2,CO and H2O at equilibrium

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