Asealed isothermal container initially contained 2 moles of co gas and 3 moles of h2 gas. the following reversible reaction occured: co(g) + 2h2(g) > ch3oh(g). at equilibrium, there was 1 mole of ch3oh in the container. what was the total number of moles of gas present in the container at equilibrium.
a.) 1
b.) 2
c.) 3
d.) 4

(c) Total Number of moles = 3

Explanation:

To solve this question we have to follow the stoichiometry of the reaction and the fact that at equilibrium we have 1 mol of CH₃OH using the mnemonic helper RICE ( Reaction, Initial, Change, Equilibrium) as follows:

R             CO(g) + 2 H₂ (g)   ⇄  CH₃OH (g)

I (mol)        2             3                     0

C (mol)       -x         x -2x               + x

E (mol)      2-x        3-2x                   x

But we are told that at equilibrium x = mol CH₃OH = 1 , then at equilibrium we will have

E (mol)       2-(1)      3-2(1)             1

E (mol)          1            1                 1

Therefore, the total number of moles of gas present in the container at equilibrium was 3

it should be p1 v1 = p2 v2

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