Question

Sample of gas initially occupies 4.25 L at a pressure of 0.850 atm at 23.0°C. What will the volume be if the temperature is changed to 11.5°C, and the pressure is changed to 1.50 atm?

Answer 1

Answer: 2.34 L

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 = 0.850 atm

`P_2` = final pressure of gas = 1.50 atm

`V_1` = initial volume of gas = 4.25 L

`V_2` = final volume of gas = ?

`T_1` = initial temperature of gas =
`23.0^oC=273+23.0=293.0K`

`T_2` = final temperature of gas =
`11.5^oC=273+11.5=284.5K`

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

`(0.850* 4.25)/(293.0K)=(1.50* V_2)/(284.5)`

`V_2=2.34L`

Thus the final volume will be 2.34 L