Question

A sample of gas contains 0.1400 mol of CH4(g) and 0.2800 mol of O2(g) and occupies a volume of 14.9 L. The following reaction takes place: CH4(g) + 2O2(g)CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

______L

Answer #1

According to reaction 1 mole CH_{4} react with 2 mole
O_{2} give 1 mole of CO_{2} and 2 mole of
H_{2}O therefore

in the reactant 0.1400 mole CH_{4} react with 0.2800
mole O_{2} give 0.14 mole of CO_{2} and 0.2800 mole
of H_{2}O

total mole of reactant = 0.1400 + 0.2800 = 0.4200 mole

total mole of product = 0.1400 + 0.2800 = 0.4200 mole

no. of mole of reactant gas = no. of mole of product gas therefore at same tempreture and pressure product gas occupy volume = reactant gas = 14.9 L

volume of the sample after the reaction takes place = 14.9 L

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N2(g) +
2O2(g)
2NO2(g)
Calculate the volume of the sample after the reaction takes place,
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