For the reaction
`CO(g)+2H_(2)(g)hArrCH_(3)OH(g)`
Hydrogen gas is introduced into a five-litre flask at `327^(@)C`, containing `0.2` mol of `CO(g)` and a catalyst, untill the pressure is `4.92 atm`. At this point, `0.1` mol of `CH_(3)OH(g)` is formed. Calculate the equilibrium constants `K_(p)` and `K_(c )`.

For the reaction CO(g)+2H_(2)(g) hArr CH_(3)OH(g) hydrogen gas is introduced into a 5-L flask at 327^(@)C containing 0.2 mol of CO(g) and a catalyst, untill the pressure is 4.92 atm. At this point, 0.1 mol of CH_(3)OH(g) is formed. Calculate the equilibrium constant K_(p) and K_(c) .

For the equilibrium system : CO(g)+2H_2(g)hArr CH_3OH(l) what is K_c ?

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 .

0.25 mol of CO taken in a 1.5 L flask is maintained at 500 K along with a catalyst so that the following reaction can take place: CO(g)+H_(2)(g)hArrCH_(3)OH(g) . Hydrogen is introduced until the total pressure of the system is 8.2 atm , at equilibrium, and 0.1 mol of methanol is formed. Calculate a. K_(p) and K_(c ) b. The final pressure if the same amount of CO and H_(2) as before are used but no catalyst so that the reaction does take place.

0.25 mol of CO taken in a 1.5 L flask is maintained at 500 K along with a catalyst so that the following reaction can take place: CO(g)+H_(2)(g)hArrCH_(3)OH(g) . Hydrogen is introduced until the total pressure of system is 8.2 atm , at equilibrium, and 0.1 mol of methanol is formed. Calculate a. K_(p) and K_(c ) b. The final pressure if the same amount of CO and H_(2) as before are used but no catalyst so that the reaction does take place.

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) 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 .