# Question 52ade

Nov 26, 2015

The final volume of nitrogen gas will be $\text{528 mL}$.

#### Explanation:

Use the combined gas law with the equation $\frac{{P}_{1} {V}_{1}}{{T}_{1}} = \frac{{P}_{2} {V}_{2}}{{T}_{2}}$.

Given/Known
${P}_{1} = \text{740 torr}$
${V}_{1} = \text{500. mL}$
${T}_{1} = \text{25"^"o""C"+273.15="298 K}$
${P}_{2} = \text{760 torr}$
${T}_{2} = \text{50"^"o""C"+273.15="323 K}$

Unknown
${V}_{2}$

Equation
$\frac{{P}_{1} {V}_{1}}{{T}_{1}} = \frac{{P}_{2} {V}_{2}}{{T}_{2}}$

Solution
Rearrange the equation to isolate ${V}_{2}$ and solve.

${V}_{2} = \frac{{P}_{1} {V}_{1} {T}_{2}}{{T}_{1} {P}_{2}}$

V_2=(740cancel"torr"xx500. "mL"xx323cancel"K")/(298cancel"K"xx760cancel"torr")="528 mL N"_2"#