Question

A sample of Hydrogen$\left(H_2\right)$gas at $127°C$has a pressure of $2.00atm$. at final temperature, in degrees Celcius, will the pressure of the $H_2$decreases to $0.25atm$, if $Vandn$do not change?

Short answer

The final temperature of$H_2$will be$-223°C$.

Step-by-step solution

Given Information

We have given the temperature is $127°C$and pressure is $2.00atm$of Hydrogen$\left(H_2\right)$.

Simplify

According to the question, there will be no change in the amount of gas and the volume of the gas will also be constant.

Using combined gas law

$\frac{p_1{V}_1}{T_1}=\frac{p_2{V}_2}{T_2}$

We can see, the pressure is directly related to the temperature.

So,

role="math" localid="1652528887995" $$\begin{gathered} T_2=\frac{P_2{T}_2}{P_1}=\frac{0.25atm\times 400K}{2atm} \\ {T}_2=50K \\ {T}_2=\left(50-273\right)°C=-223°C \end{gathered}$$