Home
Class 11
CHEMISTRY
An equilibrium mixture CO(g)+H(2)O(g) ...

An equilibrium mixture
`CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g)`
present in a vessel of one litre capacity at `815^(@)C` was found by analysis to contain `0.4` mol of CO, `0.3` mol of `H_(2)O, 0.2` mol of `CO_(2)` and `0.6` mol of `H_(2)`.
a. Calculate `K_(c)`
b. If it is derived to increase the concentration of CO to `0.6` mol by adding `CO_(2)` to the vessel, how many moles must be addes into equilibrium mixture at constant temperature in order to get this change?

Promotional Banner

Similar Questions

Explore conceptually related problems

An equilibrium mixture CO(g) + H_(2) O (g) hArr CO_(2) (g) + H_(2) (g) present in a vessel of one litre capacity at 1000 K was found to contain 0*4 mole of CO, 0*3 mole of H_(2)O, 0*2 mole of CO_(2) and 0*6 mole of H_(2) . If it is desired to increase the concentration of CO to 0*6 mole by adding CO_(2) into the vessel , how many moles of it must be added into equilibrium mixture at constant temperature in order to get this change ?

The reaction, CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300 K in a 1 L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant K_(c ) for the reaction at the given temperature us 3.90 .

The reaction, CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300 K in a 1 L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant K_(c ) for the reaction at the given temperature us 3.90 .

The reaction CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300K in a 1L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_2O and an unknown amount of CH_(4) in the flask. Determine the concentration on CH_(4) in the mixture. the equilibrium constant, K_(c) for the reaction at the given temperature is 3.90.

The reaction , CO(g)+3H_(2)(g)hArrCH_(4)(g)+H_(2)(g) is at equilibrium at 1300K in a 1L flask. It also contain 0.30 mol of CO , 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant. K_(c) for the reaction at the given temperature is 3.90 .

In the following system at equilibrium, N_(2)+3H_(2)hArr2NH_(3) , the reaction mixture contains 0.005 mol of N_(2) , 0.012 mol of H_(2) and 0.002 mol of NH_(3) in a 2 litre vessel. Calculate K_(c) .

The reaction : CO(g)+3H_2(g)hArr CH_4(g) +H_2O(g) is at equilibrium at 1300 K in a one litre flask. The gaseous equilibrium mixture contains 0.30 mol of CO, 0.10 mol of H_2 and 0.020 mol of H_2O and an unknown amount of CH_4 in the flask. Determine the concentration of CH_4 in the mixture . The equilibrium consant K_c for the reaction at given temperature is 3.90