Gaseous methane (ch4) reacts with gaseous oxygen gas (o2) to produce gaseous carbon dioxide (co2) and gaseous water (h2o). what is the theoretical yield of water formed from the reaction of 101. g of methane and 53.2 g of oxygen gas? be sure your answer ha

CH4 + 2O2 → CO2 + 2H2O

M(CH4) = 16.04 g/mol

n(CH4) "= \\frac{6.3}{16.04}=0.393 \\;mol"

M(O2) = 15.99 g/mol

n(O2) "= \\frac{15.0}{15.99}=0.938 \\;mol"

For each mole of CH4 we need only 2 moles of O2, but for 0.393 mol of CH4 we have more O2 than needed. So, CH4 is the limiting reactant.

According to the reaction:

n(H2O) = 2n(CH4) "= 2 \\times 0.393 = 0.786 \\;mol"

M(H2O) = 18.01 g/mol

m(H2O) "= 18.01 \\times 0.786 = 14.15 \\;g"

Answer: 14.1 g.

Get the answer to your homework problem.

Try Numerade free for 30 days

Case Western Reserve University

John N.

Chemistry 101

5 months, 2 weeks ago

We don’t have your requested question, but here is a suggested video that might help.

Gaseous methane $\left(\mathrm{CH}_{4}\right)$ undergoes complete combustion by reacting with oxygen gas to form carbon dioxide and water vapor. a. Write a balanced equation for this reaction. b. What is the volume ratio of methane to water in this reaction?

Get the answer to your homework problem.

Try Numerade free for 30 days

Nicholas H.

Chemistry 101

4 months, 2 weeks ago