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
mm Hg.
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.