The reaction, `CO(g) + 3H_2 (g) hArr CH_4(g) + H_2O(g)` is at equilibrium at 1300K in a 1L.flask.If also contain 0.30 mol of CO. 0.10 mol of `H_2` and 0.02 mol of `H_2O ` and unkown amount of `CH_4` in the flask.Determine the concentration of `CH_4` in the mixture.
The quilibrium constant.`K_c` for the reacton at the given temperature is 3.90.

Describe the effect of : addition of H_2 on the eauilibrium of the reaction, 2H_2(g) + CO(g) hArr CH_3OH(g)

Describe the effect of :addition of CH_3OH on the eauilibrium of the reaction, 2H_2(g) + CO(g) hArr CH_3OH(g)

Describe the effect of :removal of CH_3OH on the eauilibrium of the reaction, 2H_2(g) + CO(g) hArr CH_3OH(g)

How many g of H_2O are present in 0.25 mol of it?

How many g of H_2 O are present in 0.25 mol of it ?

Given the reaction, CH_2O_((g))+ O_(2(g)) rarr CO_(2(g))+H_2O_((g)) DeltaH=- 527 kJ How much heat will be evolved in the formation of 30 g of CO_2 ?

Equilibrium constant, K_c for the reaction, N_2(g) +3H_2(g) hArr 2NH_3(g) _(at 500 k is 0.061) At a particular time, the analysis shows that composition of the reaction mixtue is 3.0 mol L^(-1) N_2,2.0 mol L^(-1) H_2 .5 mol L^(-1) NH_3 Is the eaction at equilibrium ?If not in which direction does the reaction tend to proceed to reach equilibrium?

At 700 K , equilibrium constant for the reaction, H_2(g) + I_2(g) hArr 2HI(g) is 54.8 if 0.5 mol L^(-1) of HI(g) is present at equilibrium at 700K,what are the concentration of H_2(g) and I_2(g) assuming that we initially started with HI(g) and allowed it to reach equilibrium at 700K?