Ch. Ex. 38- Ideal Gas Law: Solve for Moles Enter your answer in the provided box

Question

Ch. Ex. 38- Ideal Gas Law: Solve for Moles Enter your answer in the provided box. In preparation for a demonstration, your professor brings a 1.50-L bottle of sulfur dioxide into the lecture hall before class to allow the gas to reach room temperature. If the pressure gauge reads 246 psi and the lecture hall is 24°C, how many moles of sulfur dioxide are in the bottle? In order to solve this problem, you will first need to calculate the pressure of the gas. Hint: The gauge reads zero when 14.7 psi of gas remains. mol

Explanation / Answer

volume V = 1.50 L

temperature = 24 + 273 =297 K

pressure of gas = 246 - 14.7 = 231.3 psi

1 atm = 14.6959 psi

x atm = 231.3 psi

x = 231.3 / 14.6959 atm = 15.73 atm

P =15.73 atm

R = 0. 0821 L atm /mol K

P V = n R T

15.73  x 1.50 = n x 0.0821 x 297

n = 0.96

moles of gas = 0.96

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