Question

A gas has a volume of 36.0 L and a pressure of 750. torr when the temperature is 10. °C. What is the pressure if the volume changes to 15.0 L and the temperature changes to 78 °C, if the amount of gas stays the same?

Answer 1

Answer: 2232 torr

Step-by-step explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

`(P_1V_1)/(T_1)=(P_2V_2)/(T_2)`

where,

`P_1` = initial pressure of gas = 750 torr

`P_2` = final pressure of gas = ?

`V_1` = initial volume of gas = 36.0 L

`V_2` = final volume of gas = 15.0 L

`T_1` = initial temperature of gas =
`10^oC=273+10=283K`

`T_2` = final temperature of gas =
`78^oC=273+78=351K`

Now put all the given values in the above equation, we get:

`(750* 36)/(283)=(P_2* 15.0)/(351)`

`P_2=2232torr`

The pressure will be 2232 torr if the volume changes to 15.0 L and the temperature changes to 78 °C, if the amount of gas stays the same.