For the reaction h2(g) + co2(g) ⇌ h2o(g) + co(g) at 700ºc, kc = 0.534. calculate the number of moles of h2 that are present at equilibrium if a mixture of 0.300 mole of co and 0.300 mole of h2o is heated to 700ºc in a 10.0-l container.

There are 173.3 moles of hydrogen gas in the container.

Explanation:

⇄ at 700ºC.

Equilibrium constant of the reaction =

If a mixture of 0.300 mole of CO and 0.300 mole of is heated to 700ºC.

Concentration of  CO=

Concentration of

    ⇄

t = 0     30 M   30M                          

at eq'm  (30 M -x)     (30 M -x)                    x    x

Equilibrium constant of the reaction =

x  = 17.33 M =

Moles of hydrogen gas

There are 173.3 moles of hydrogen gas in the container.

Explanation:

Hello,

In this case, for the given reaction, the law of mass action turns out:

In such a way, the reactants initial concentrations are:

And considering the change due to the equilibrium, the law of mass action takes the following form:

The feasible answer is

Therefore, the hydrogen moles at equilibrium are:

Best regards.

11 players on a field that has a maximum of 11 players