Chapter 5, Problem 5.94P

Methanol ${\text{(CH}}_{\text{4}}\text{O),}$ which is used as a fuel in high-performance racing cars, burns in the presence of O₂ to form CO₂ and H₂O. The molar masses for all substances are given under the balanced equation.

   ${\text{2CH}}_{\text{4}}\text{O(l) }+3{\text{O}}_{\text{2}}(g)\to 2{\text{CO}}_{\text{2}}{\text{(g), + 4H}}_{\text{2}}\text{O(g)}$

   $\text{32}\text{.04 g/mol 32}\text{.00 g/mol 44}\text{.01 g/mol 18}\text{.02 g/mol}$

1. What is the theoretical yield of CO₂ from 48.0 g of methanol?
2. What is the percent yield of CO₂ if 48.0 g of CO₂ are formed?