Answer:
602.95 kPa.
Explanation:
- To solve these problems, we can use the general law of ideal gas: PV = nRT.
where, P is the pressure of the gas in atm.
V is the volume of the gas in L (V = 39.0 L).
n is the no. of moles of the gas in mol.
R is the general gas constant (R = 0.082 L.atm/mol.K).
T is the temperature of the gas in K (T = 19.0 °C + 273.15 = 292.15 K).
The volume of the gas = nRT/P.
P = ??? atm, V = 39.0 L, R = 0.082 L.atm/mol.K, n = mass/molar mass = (310.0 g)/(32.0 g/mol) = 9.6875 mo, T = 19.0 °C + 273.15 = 292.15 K.
∴ P = nRT/V = (9.6875 mol)(0.082 L.atm/mol.K)(292.15 K)/(39.0 L) = 5.95 atm.
- To convert fom atm to kPa:
101.325 kPa = 1.0 atm.
∴ P = 5.95 atm x (101.325 kPa / 1.0 atm) = 602.95 kPa.
