1.30 mol sample of krypton gas at a temperature of 17.0 °C is found to occupy a volume of 24.7 liters. The pressure of this gas sample is

Question

mm Hg.

Answer 1

To find the pressure of the gas sample, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure
V = volume (24.7 L)
n = number of moles (1.30 mol)
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (17.0°C + 273.15 = 290.15 K)

Now we can plug in the values:

P(24.7) = (1.30)(0.0821)(290.15)

P(24.7) = 31.8969

P ≈ 31.8969 / 24.7
P ≈ 1.29 atm

To convert atm to mm Hg, we can use the conversion factor:
1 atm = 760 mm Hg

So, 1.29 atm x 760 mm Hg = 979.4 mm Hg

Therefore, the pressure of the krypton gas sample is approximately 979.4 mm Hg.