Hello, Emma,
There is no change in the volume nor in the number of moles.
With no change in the moles, we can use the gas law in this format:
P1V1/T1 = P2V2/T2
Where P, V, and T are the pressure, volume, and temperature at the initial (1) and final (2) states. Temperature must be in degrees Kelvin (add 273.15 to C). Rearrange to find the unknown, P2.
P2 = P1(V1/V2)(T2/T1)
Since the volume does not change, this simplifies to:
P2 = P1(V1/V2)(T2/T1)
P2 = P1(T2/T1)
Convert the temperatures to degrees K (300.15K and 350.15K). Put these two values into the equation, add P1 and then calculate. Before you do, predict what will happen to the temperature. We are heating a gas in a closed container. The volume remains the same as do the moles of gas. The gas has nothing to do but increase pressure.
Calculate these values and be sure that the units cancel except for atm, the pressure. I get 8.63 atm. Make that 8.6 atm for 2 sig figs.
Bob
I get
