A cylinder contains 12.4 L of air at a total pressure of 41.4 psi and a...
A cylinder contains 12.4 L of air at a total pressure of 41.4 psi and a temperature of 35 ∘C. How many moles of gas does the cylinder contain? (Hint: You must convert each quantity into the correct units (L, atm, mol, and K) before substituting into the ideal gas law.)
Homework Answers
P = 41.4 psi = 41.4×0.068 atm = 2.82 atm
(1psi = 0.068 atm)
V = 12.4 L
T = 35°C = 35 + 273.15 K = 308.15 K
R = 0.082 Latm/mol.K
n = PV/RT = 2.82×12.4/(0.082×308.15) mol
= 1.38 mol
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