1 answer

A cylinder contains 12.6 L of air at a total pressure of 41.4 psi and a...

Question:

A cylinder contains 12.6 L of air at a total pressure of 41.4 psi and a temperature of 25C Part A How many moles of gas does
A cylinder contains 12.6 L of air at a total pressure of 41.4 psi and a temperature of 25C Part A 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.) Express your answer with the appropriate units HAO? oring Value Units Submit Request Answer

Answers

According to given data:

A cylinder contain,

Volume(V) = 12.6 L , Pressure(P) = 41.4psi, and Temperature(T) = (25 + 273)K = 298 K P = 41.4psi = 41.4 * 0.068atm = 2.8152atm

According to ideal gas:

PI n = RT

n = 2.8152atm * 12.6L 0,0821atm. L.mol-.K-298K 35.47 24.46

n = 1.45mol

.

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