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[" 4.The equilibrium constant "K(p)" for...

[" 4.The equilibrium constant "K_(p)" for the reaction "],[qquad H_(2)(g)+CO_(2)(g)rightleftharpoons H_(2)O(g)+CO(g)],[" is "4.0" at "1660^(@)C" .Initially "0.80" mole "H_(2)" and "0.80moleCO_(2)" are injected into a "5.0" litre flaye "],[" is "4.0" at "1660^(@)C" .Initially "0.80" mole "H_(2)" and "0.80moleCO_(2)" are injected into a "5.0" litre flay,"],[" What is the equilibrium concentration of "CO_(2)(g)" ? "],[[" (a) "0.533M," (b) "0.0534M," (c) "0.535M," (d) None of these "]]

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The equilibrium constant K_(p) for the reaction H_(2)(g)+CO_(2)(g)hArrH_(2)O(g)+CO(g) is 4.0 at 1660^(@)C Initially 0.80 mole H_(2) and 0.80 mole CO_(2) are injected into a 5.0 litre flask. What is the equilibrium concentration of CO_(2)(g) ?

The equilibrium constant K_(p) for the reaction H_(2)(g)+CO_(2)(g)hArrH_(2)(g)+CO(g) is 4.0 at 1660^(@)C Inittally 0.80 H_(2) and 0.80 mole CO_(2) are injecteed into a 5.0 litre flask what is the equilibrium concentraton of CO_(2)(g) ?

The equilibrium constant K_(p) for the reaction H_(2)(g)+CO_(2)(g)hArrH_(2)(g)+CO(g) is 4.0 at 1660^(@)C Inittally 0.80 H_(2) and 0.80 mole CO_(2) are injecteed into a 5.0 litre flask what is the equilibrium concentraton of CO_(2)(g) ?

The equilibrium constant for the reaction , H_(2) (g) + CO_(2) (g) hArr H_(2) O (g) + CO (g) is 16 at 1000^(@) C . If 1.0 mole of H_(2) and 1.0 mole of CO_(2) are placed in one litre flask , the final equilibrium concentration of CO at 1000^(@) C is

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be

The value of K for H_(2)(g)+CO_(2)(g)hArr H_(2)O(g)+CO(g) is 1.80 at 1000^(@)C . If 1.0 mole of each H_(2) and CO_(2) placed in 1 litre flask, the final equilibrium concentration of CO at 1000^(@)C will be

At a given temperature, Kc is 4 for the reaction: H_2(g)+CO_2(g) ⇔H_2O(g)+CO(g) .Initially 0.6 moles each of H_2 and CO_2 are taken in 1 liter flask. The equilibrium concentration of H_2O(g) is :

The equilibrium constant for, H_2(g) +CO_2(g) hArr H_2O(g) + CO(g) is 1.80 at 1000^Oc . If 1.0 mole of H_2 and 1.0 mole of CO_2 are placed in one litre flask. What will be the final equilibrium concentration of CO at 1000^Oc ?