Question

The temperature of a sample of dinitrogen monoxide is changed with constant volume, causing a change in pressure from 11.5 atm to 3.3 atm. If the starting temperature was 446.5 K, what is the final temperature in Kelvins?

Answer 1

Explanations:

According to the Gay's Lussac's law, the pressure of a given mass of gas is directly proportional to the temperature provided that the volume is constant. Mathematically;

`\begin{gathered} P\alpha T \\ P=kT \\ k=(P_1)/(T_1)=(P_2)/(T_2) \end{gathered}`

Given the following parameters

Initial pressure P1 = 11.5atm

Final pressure P2 = 3.3atm

Initial temperature T1 = 446.5K

Required

Final temperature T2

Substitute the given parameters into the formula

`\begin{gathered} T_2=(P_2T_1)/(P_1) \\ T_2=(3.3*446.5)/(11.5) \\ T_2=128.13K \end{gathered}`

Hence the final temperature in kelvins is 128.13K