Question

Hydrogen gas is produced industrially by reacting methane gas, CH4 (g), with water vapor to from carbon monoxide and hydrogen gas. In a particular reaction, 25.5L of methane (measured at a pressure of 732 torr and a temperature of 25degree Celcius) mixes with 22.8 L of water vapor(measured at a pressure of 702 torr and a temperature of 125 degree Celcius). What is the theoretical yield hydrogen gas at STP? Give your answer in units of L to three significant figures.
bobpursley
write the balanced equation:
CH4+H2O >> 3H2 + CO
get all the reactants moles:
CH4: n=PV/RT=732*25.5/R(298)=62.6/R
H2O: n=22.8*702/R(398)=40.2/R
so you have an excess of CH4.
So according to the balanced equation, you will get moles of H2 of 3*40.2/R =121/R moles H2
of volume determined by
V=nRT/P=121/R * R*273/760=43.7L

check my work.

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