Question

Helium gas in a cylinder is under 1.12atm pressure at 25.0C. What will be the pressure if the temperature increases to 37.0C?

Answer 1

`p_2=1.17atm`

Step-by-step explanation:

Hello!

In this case, considering that the Gay-Lussac's law allows us to relate the temperature-pressure problems as directly proportional relationships:

`(p_2)/(T_2) =(p_1)/(T_1) \\\\`

Thus, for the initial pressure and temperature in kelvins the final temperature in kelvins, we compute the final pressure as:

`p_2=(p_1T_2)/(T_1) \\\\p_2=(1.12atm*310.15K)/(298.15K)\\\\p_2=1.17atm`

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