Question

A gas sample has an original volume of 580 ml when collected at 1.20 atm and 22oC. If a change is made in the gas pressure which causes the volume of the gas sample to become 1.45 liters at 40oC, what is the new pressure?

Answer 1

Answer: The new pressure is 0.509 atm

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 = 1.20 atm

`P_2` = final pressure of gas = ?

`V_1` = initial volume of gas = 580 ml

`V_2` = final volume of gas = 1.45 L = 1450 ml (1L=1000ml)

`T_1` = initial temperature of gas =
`22^0C=(22+273)K=295K`

`T_2` = final temperature of gas =
`40^0C=(40+273)K=313K`

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

`(1.20* 580)/(295)=(P_2* 1450)/(313)`

`P_2=0.509atm`

The new pressure is 0.509 atm