`K_(c )` for `CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)` at `986^(@)C` is `0.63`. A mixture of `1` mol `H_(2)O(g)` and `3` mol `CO_(2)(g)` is allowed to react to come to an equilibrium. The equilibrium pressure is `2.0` atm.
a. Hoe many moles of `H_(2)` are present at equilibrium ?
b. Calculate partial pressure of each gas at equilibrium.

K_(c ) for CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) at 986^(@)C is 0.63 . A mixture of 1 mol H_(2)O(g) and 3 mol CO (g) is allowed to react to come to an equilibrium. The equilibrium pressure is 2.0 atm. a. How many moles of H_(2) are present at equilibrium ? b. Calculate partial pressure of each gas at equilibrium.

A mixture of 4 moles H_(2)O and 1 mole CO is allowed to react to come to an equilibrium. The equilibrium pressure is 2.0 atm. Calculate partial pressure (in atm) of CO(g) at equilibrium. H_(2)O (g) + CO(g) harr CO_(2) (g) + H_(2) (g); K_(C) =0.5 Use sqrt(41) = 6.4

At 986^(@) C the value of equilibrium constant (K_c) for the reaction, CO(g)+H_2O(g)toCO_2(g)+H_2(g) is 0.63At this temperature, 1 mol of H_2O (g) is allowed to react with 3 mol of CO(g). This results in the above equilibrium in which the observed pressure is 2.0 atm. Find the number of moles of H_2 (g) produced at equilibrium and the partial pressure of each gas

H_(2)(g) + I_(2)(g)hArr2HI(g) When 46 g of I_(2) and 1 g of H_(2) gas heated at equilibrium at 450^(@)C , the equilibrium mixture contained 1.9 g of I_(2) . How many moles of I_(2) and HI are present at equilibrium ?

At 675 K, H_(2)(g) and CO_(2)(g) react to form CO(g) and H_(2)O(g), K_(p) for the reaction is 0.16. If a mixture of 0.25 mole of H_(2) (g) and 0.25 mol of CO_(2) is heated at 675 K, mole% of CO(g) in equilibrium mixture is :

For the reaction CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) at a given temperature, the equilibrium amount of CO_(2)(g) can be increased by

For the reaction CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) at a given temperature, the equilibrium amount of CO_(2)(g) can be increased by

For the reaction CO(g) +H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) at a given temperature the equilibrium amount of CO_(2) (g) can be increased by