a newconnect.mheducation.com Connect iters of th Park-S21 (2016)-Episode 10 Free

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a newconnect.mheducation.com Connect iters of th Park-S21 (2016)-Episode 10 Free On Sol.. Chapter Five: Gases and the Kinetic-Molecular The... . 9 Ch. Ex. 38-Ideal Gas Law: Solve for Moles 10 points 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 reom temperature. If the pressure gauge reads 398 psi and the lecture hall is 25°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 02 44 20 mol

Explanation / Answer

Pressure of gas = 398 - 14.7 = 383.3 psi = 383.3 * 0.0680 atm = 26.1 atm

V = 1.50 L

T = 25 + 273.15 = 298.15

R = 0.0821 L.atm.K-1.mol-1

n = ?

Using ideal gas equation,

P V = n R T
n = 26.1 * 1.50 / (0.0821 * 298.15)

n = number of moles of SO2 in the bottle = 1.60 mol

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