Question

Find the amount of oxygen required for the complete combustion of 4 mol of butane.
$2C_4{H}_{10}+13O_2\to 8C{O}_2+10H_{2}O$

• A. $832\text{g}$
• B. $416\text{g}$
• C. $280\text{g}$
• D. $530\text{g}$

Answer 1

The correct option is A $832\text{g}$

$2C_4{H}_{10}+13O_2\to 8C{O}_2+10H_{2}O$

2 mol of $C_4{H}_{10}$ require 13 mol of $O_2$
So, 4 mol of $C_4{H}_{10}$ will require = $\frac{13}{2}\times 4$ = 26 mol of $O_2$

Mass of oxygen required = $26\text{mol}\times 32\text{g/mol}$
Mass of oxygen required = $832\text{g}$