Question

A gas has a pressure of 1.34 atm when the temperature is 237K. The gas is then

Answer 1

Answer:

$\large \boxed{\text{1.76 atm}}$

Explanation:

The volume and amount of gas are constant, so we can use Gay-Lussac’s Law:

At constant volume, the pressure exerted by a gas is directly proportional to its temperature.

$\dfrac{p_{1}}{T_{1}} = \dfrac{p_{2}}{T_{2}}$

Data:

p₁ = 1.34 atm; T₁  = 237 K

p₂ = ?;             T₂ = 312 K

Calculations:

$\begin{array}{rcl}\dfrac{1.34}{237} & = & \dfrac{p_{2}}{312}\\\\5.654 \times 10^{-3} & = & \dfrac{p_{2}}{312}\\\\5.654 \times 10^{-3}\times312&=&p_{2}\\p_{2} & = & \textbf{1.76 atm}\end{array}\\\text{The new pressure will be \large \boxed{\textbf{1.76 atm}} }$