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24 December, 21:11

If a 3.00-l flask contains 0.400 mol of co2 and 0.100 mol of o2 at equilibrium, how many moles of co are also present in the flask?

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  1. 24 December, 22:50
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    When the balanced equation for this reaction is:

    2CO (g) + O2 (g) → 2CO2 (g)

    and according to Kc formula = concentration of the products/concentration of the reactant

    Kc = [CO2]^2 / [CO]^2 [O2]

    by getting the concentration of CO2 = 0.4 (no. of moles) / 3 (volume per L) = 0.13

    and the concentration of O2 = 0.1 (no. of moles of O2) / 3 (volume per L) = 0.03

    and we have Kc value (given) = 1.4 x 10^2

    So by substitution in the Kc formula:

    1.4x10^2 = 0.13^2 / [Co]^2 * 0.03

    [CO]^2 = 0.13^2 / (1.4x10^2 * 0.03) = 0.004

    [CO] = √0.004 = 0.63

    that means moles of CO = 0.63 x 3 (volume L) = 1.89 moles
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