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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Aakash · Answer

atreyee · Answer

Here K p = K c . Taking dissociation constant as a, ((3a) 2 /(3(1-a)) 2 )=0.137 Solving for a, =0.27. Hence equillibrium concentrations of CO and H 2 O are 1.5+.81=2.31moles/L each and that of CO 2 and H 2 are 2.19moles/L each.

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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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