Chapter 5, Problem 5.53E

Suppose you want to use acetylene $\left({\text{C}}_{\text{2}}{\text{H}}_{\text{2}}\right)$ as a fuel. You have a cylinder that contains $5.00\times {10}^2\text{g}$ of ${\text{C}}_{\text{2}}{\text{H}}_{\text{2}}$ and a cylinder that contains $2.00\times {10}^3\text{g}$ of oxygen $\left({\text{O}}_{\text{2}}\right)$. Do you have enough oxygen to burn all the acetylene? The equation for the reaction is

${\text{2C}}_{\text{2}}{\text{H}}_{\text{2}}\left(\text{g}\right)+5{\text{O}}_{\text{2}}\left(\text{g}\right)\to 4{\text{CO}}_{\text{2}}\left(\text{g}\right)+2{\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)$