QUESTION 15 The partial pressures of CH4, N2, and O2 in a sample of gas were fou

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QUESTION 15 The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 155 mmHg, 476 mmHg and 669 mmHg, respectively. What is the mole fraction of nitrogen? A. 0.410 B. 20.9 C. 0880 D.0.515 E, 0.366 QUESTION 16 What volume of ammonia gas, measured at 660.3 mmHg and 58.2°C, is required to produce 6.46 g of ammonium sulfate according to the following balanced chemical equation? 2NHyun-H2SO4(aq) ? (NH4)2SO4(s) C.0765 L D. 11.9L 0.00312 L Click Save and Submit to save and submit Click Save AN Answers to save al answers O Type here to search

Explanation / Answer

Question 15

According to Raoult's law: PN2 = P * xN2, where xN2 is the mole fraction of nitrogen.

P = PCH4 + PN2 + PO2

i.e. P = 155 + 476 + 669 = 1300 mm Hg

Now, 476 = 1300*xN2

i.e. xN2 = 476/1300 = 0.366 (Option E)

Question 16

Given data: Pressure (P) = 660.3 mm Hg = 660.3/760 atm = 0.8688 atm

T = 58.2 oC = (58.2 + 273.15) K = 331.35 K

The no. of moles of (NH4)2SO4 (n) = 6.46 g/132 g mol-1 = 0.0489 mol

Universal gas constant (R) = 0.08206 L atm mol-1 K-1

According to ideal gas equation: PV = nRT

i.e. 0.8688 atm * V = 0.0489 mol * 0.08206 L atm mol-1 K-1 * 331.35 K

i.e. The volume of ammonium sulfate (V) = 1.53 L

According to the balanced equation, the volume of ammonia gas = 2*1.53 = 3.06 L (Option B)

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