# Question a9607

Jul 7, 2017

$4.0 \times {10}^{2}$ $\text{K}$

#### Explanation:

We can use the ideal gas equation to solve this problem:

$P V = n R T$

where

• $P$ is the pressure exerted by the gas, in $\text{atm}$

• $V$ is the volume occupied by the gas, in $\text{L}$

• $n$ is the number of moles of gas present

• $R$ is the universal gas constant, equal to $0.082057 \left(\text{L"•"atm")/("mol"•"K}\right)$

• $T$ is the absolute temperature of the gas, in $\text{K}$

Since all our units are appropriate, let's plug things in and solve for $T$:

$T = \frac{P V}{n R}$

= ((1.5cancel("atm"))(12.9cancel("L")))/((0.59cancel("mol"))(0.082057(cancel("L")•cancel("atm"))/(cancel("mol")•"K"))) = color(red)(4.0xx10^2 color(red)("K"#

rounded to two significant figures.