A gas at 0.98 atm and 35 oC is heated to 96 oC. Assuming there is no change in volume, what is the new pressure in atm?

Answer 1

Hello, Reyes,

Since there is no change in the moles of gas, we can use a simplified gas law:

P1V1/T1 = P2V2/T2

The initial Pressure, Volume, and Temperature are designated with the subscript "1." The final values have the subscript "2." Temperatures need to be entered in Kelvin, so add 273 to each of the Cent. values.

We are also told there is no change in volume, so V1 = V2 and we can reduce the equation even further and rearrange to find P2:

P2 = P1(T2/T1)

Enter the data: P2 = 0.98atm*((96+273K)/(35+273K)

That comes out around 1.17 atm. It should be higher, since the temperature rose but the volume was constrained.

I hope this helps,

Bob

Answer 2

P1 / T2 = P2 / T2

T1= 35C + 273 =308K

T2= 96C + 273 = 369K

0.98atm / 308k = P2 / 369K

P2 = 0.98atm x 369K / 308K

P2 = 1.174 atm