At 87°C, the following equilibrium is established `H_(2)(g) + S(s)hArrH_(2)S(g) K_(p) = 7 x× 10^(-2)`. If 0.50 mole of hydrogen and 1.0 mole of sulfur are heated to 87°C in 1.0 L vessel, what will be the partial pressure of `H_(2)S` at equilibrium ?

At 87^(@)C , the following equilibrium is established H_(2) (g)+S(s)hArrH_(2)(g), K_(p)=7xx10^(-2) If 0.50 mole of hydrogen and 1.0 mole of sulphur are heated to 87^(@)C in 1 L vessel. What is the partial pressure of H_(2)S (g) at equilibrium?

At 87^(@)C , the following equilibrium is established H_(2) (g)+S(s)hArrH_(2)S(g), K_(p)=7xx10^(-2) If 0.50 mole of hydrogen and 1.0 mole of sulphur are heated to 87^(@)C calculate partial pressure of H2S at eq.

At 87^(@)C , the following equilibrium is established. H_(2)(g)+S(s) hArrH_(2)S(g), K_(c)=0.08 If 0.3 mole hydrogen and 2 mole sulphur are heated to 87^(@)C in a 2L vessel, what will be concentration of H_(2)S at equilibrium ?

At 87^(@)C , the following equilibrium is established. H_(2)(g)+S(s) hArrH_(2)S(g), K_(c)=0.08 If 0.3 mole hydrogen and 2 mole sulphur are heated to 87^(@)C in a 2L vessel, what will be concentration of H_(2)S at equilibrium ?

At 87^(@)C , the following equilibrium is established H_(2) (g)+S(s)hArrH_(2)S(s)(g), K_(p)=7xx10^(-2) If 0.50 mole of hydrogen and 1.0 mole of sulphuur are heated to 87^(@)C and 2.0 atm .the equilibrium gases mixture contains 40% chlorine by volume. Calculate K_(p) at 247^(@)C for the reaction PCl_(5)(g)hArrPCl_(3)(G)+Cl_(2)(g)

An equilibrium mixture for the reaction 2H_2S(g) hArr 2H_2(g)+S_2(g) had 1 mole of hydrogen sulphide, 0.2 mole of H_2 and 0.8 mole of S_2 in 2 litre vessel. The value of K_c is:

An equilibrium mixture for the reaction 2H_2S (g) hArr 2H_2(g)+S_2(g) had 1 mole of hydrogen sulphide, 0.2 mole of H, and 0.3 mole of S_2 in 2 litre vessel. The value of K_c is

For the equilibrium H_(2)(g)+CO_(2)(g)hArr hArr H_(2)O(g)+CO(g), K_(c)=16 at 1000 K. If 1.0 mole of CO_(2) and 1.0 mole of H_(2) are taken in a l L flask, the final equilibrium concentration of CO at 1000 K will be

For the equilibrium H_(2)(g)+CO_(2)(g)hArr hArr H_(2)O(g)+CO(g), K_(c)=16 at 1000 K. If 1.0 mole of CO_(2) and 1.0 mole of H_(2) are taken in a l L flask, the final equilibrium concentration of CO at 1000 K will be