Answer:
[tex]\large \boxed{\text{1.76 atm}}[/tex]
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.
[tex]\dfrac{p_{1}}{T_{1}} = \dfrac{p_{2}}{T_{2}}[/tex]
Data:
p₁ = 1.34 atm; T₁ = 237 K
p₂ = ?; T₂ = 312 K
Calculations:
[tex]\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 $\large \boxed{\textbf{1.76 atm}}$}[/tex]
