Solution Found!
Answer: A mixture of methane (CH4) and ethane (C2H6) of
Chapter 3, Problem 147P(choose chapter or problem)
A mixture of methane (\(\mathrm{CH}_{4}\)) and ethane (\(\mathrm{C}_{2} \mathrm{H}_{6}\)) of mass 13.43 g is completely burned in oxygen. If the total mass of \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) produced is 64.84 g, calculate the fraction of \(\mathrm{CH}_{4}\) in the mixture.
Questions & Answers
QUESTION:
A mixture of methane (\(\mathrm{CH}_{4}\)) and ethane (\(\mathrm{C}_{2} \mathrm{H}_{6}\)) of mass 13.43 g is completely burned in oxygen. If the total mass of \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) produced is 64.84 g, calculate the fraction of \(\mathrm{CH}_{4}\) in the mixture.
ANSWER:
Step 1 of 3
The goal of the problem is to calculate the fraction of in the mixture.
Given:
Mass of mixture of methane () and ethane () = 13.43 g
Mass of and produced = 64.84 g.
The balanced equations are:
let ‘x’ be mass of and (13.43 - x) g be the mass of .
Next, let’s calculate the mass of and produced by and .