Question

A sample of a gas at 25°C has a volume of 150 mL when its pressure is 0.947 atm. What will the temperature of the gas be at a pressure of

0.987 atm and the volume changes to 144mL?
Be sure to show all of your work, define variables, show equation and substitute variables. Report you answer in Celcius.

Answer 1

Answer: The temperature of the gas at a pressure of 0.987 atm and volume of 144mL is
`25.16^0C`

Step-by-step explanation:

The combined gas equation is,

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

where,

`P_1` = initial pressure of gas = 0.947 atm

`P_2` = final pressure of gas = 0.987 atm

`V_1` = initial volume of gas = 150 ml

`V_2` = final volume of gas = 144 ml

`T_1` = initial temperature of gas =
`25^0C=(25+273.15)K=298.15K`

`T_2` = final temperature of gas = ?

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

`(0.947* 150)/(298.15)=(0.987* 144)/(T_2)`

`T_2=298.31K=(298.31-273.15)^0C=25.16^0C`

The temperature of the gas at a pressure of 0.987 atm and volume of 144mL is
`25.16^0C`