Question

Calculate the pressure, in atmospheres, of 2.80 moles helium gas in a 18.0 liters container at 24 degrees celcius.
The ideal gas law is PV = nRT. You have n (2.80mol), V (18L), and T (24°C). R is the universal gas constant (which equals 0.0821 L* atm/mol * K).

Convert Celsius to Kelvin:

24°C + 273K = 297K

insert the numbers into the equation:

P(18L) = (2.80mol)(0.0821 L atm/mol * K)(297K)

isolate P:

P = (2.80mol)(0.0821 L atm/mol * K)(297K)/(18L)


P = 0.178 atm

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