Explanation Given: The equilibrium constant for the reaction ( K p ) is 5.3 × 10 − 5 . Mass of nitrogen is 1.27 kg . Mass of hydrogen is 0.310 kg . Volume of the container ( V ) is 200 L . Temperature ( T ) is 725 K . Ideal gas constant ( R ) is 0.0821 L atm / ( mol K) . Explanation: Molar mass of nitrogen is 28.0134 g / mol . Molar mass of hydrogen is 2.016 g / mol . One kilogram is equal to thousand grams. Convert kilograms to grams 1.27 kg = 1.27 kg × 1000 g 1 kg = 1270 g 0.310 kg = 0.310 kg × 1000 g 1 kg = 310 g Calculate the number of moles of nitrogen ( n N 2 ) n N 2 = 1270 g 28.0134 g / mol = 45.335 mol Calculate the number of moles of hydrogen ( n H 2 ) n H 2 = 310 g 2.016 g / mol = 153.77 mol Now, calculate the pressure of nitrogen using the ideal gas equation P N 2 = n N 2 R T V Substitute 45.335 mol for n N 2 , 200 L for V , 725 K for T , 0.0821 L atm / ( mol K) for R . P N 2 = 45.335 mol × 0.0821 L atm / ( mol K) × 725 K 200 L = 13.5 atm Now calculate the pressure of hydrogen using the ideal gas equation. P H 2 = n H 2 R T V Substitute 153.77 mol for n N 2 , 200 L for V , 725 K for T , 0.0821 L atm / ( mol K) for R . P H 2 = 153.77 mol × 0.0821 L atm / ( mol K) × 725 K 200 L = 45.8 atm Now consider the given reaction N 2 ( g ) + 3 H 2 ( g ) ⇌ 2 NH 3 ( g ) Construct the ICE table as follows: N 2 ( g ) ( atm ) 3 H 2 ( g ) ( atm ) 2 NH 3 ( g ) ( atm ) Initial 13

Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition

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ISBN: 9780134554259

Author: Nivaldo J. Tro

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Chapter 15, Problem 83E

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To determine: Mass of NH3 present and the percent yield of the reaction mixture.

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Chapter 15, Problem 82E

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Chemistry: A Molecular Approach Selected Solutions Manual, Books a la Carte Edition

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Mass of NH 3 present and the percent yield of the reaction mixture.

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To determine: Mass of NH3 present and the percent yield of the reaction mixture.

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