Asked by Cali234
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.
Answers
Answered by
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.
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.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.