Question

(show work please) At what temperature (in kelvin) would a 700ml balloon that has a pressure of 720mmhg and contained 0.25 mol of helium be?​

Answer 1

The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin.

To solve for temperature, we rearrange the equation to T = PV/nR.

First, we need to convert the volume to liters: 700 mL = 0.7 L.

The pressure also needs to be converted to atmospheres: 720 mmHg = 0.947 atm.

Now we can plug in the values:

T = (0.947 atm)(0.7 L)/(0.25 mol)(0.08206 L·atm/mol·K)

T = 24.8 K

Therefore, the temperature of the balloon is approximately 24.8 Kelvin.