Question

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

heated until the temperature measures 312K. What will be the new pressure?

Answer 1

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

Step-by-step 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.

`(p_(1))/(T_(1)) = (p_(2))/(T_(2))`

Data:

p₁ = 1.34 atm; T₁ = 237 K

p₂ = ?; T₂ = 312 K

Calculations:

`\begin{array}{rcl}(1.34)/(237) & = & (p_(2))/(312)\\\\5.654 * 10^(-3) & = & (p_(2))/(312)\\\\5.654 * 10^(-3)*312&=&p_(2)\\p_(2) & = & \textbf{1.76 atm}\end{array}\\\text{The new pressure will be $\large \boxed{\textbf{1.76 atm}}$}`