Ammonia reacts with O 2 to form either NO( g ) or NO 2 ( g ) according to these unbalanced equations: NH 3 ( g ) + O 2 ( g ) → NO ( g ) + H 2 O ( g ) NH 3 ( g ) + O 2 ( g ) → NO 2 ( g ) + H 2 O ( g ) In a certain experiment 2.00 moles of NH 3 (g) and 10.00 moles of O 2 ( g ) are contained in a closed flask. After the reaction is complete, 6.75 moles ofO 2 ( g ) remains. Calculate the number of moles of NO(g) in the product mixture: ( Hint: You cannot do this problem by adding the balanced equations because you cannot assume that the two reactions will occur with equal probability.)

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Interpretation Introduction Interpretation: The number of moles of NO ( g ) in the product mixture is calculated. Concept introduction: The number of moles in an atom is defined as the given mass divided by the molecular mass. One mole is equal to the Avogadro’s number and each element consists of different molar mass that depends on the weight of its atom. To determine: The number of moles of NO ( g ) in the product mixture. Explanation Explanation Given The balanced chemical reactions are, 4NH 3 + 5O 2 → 4NO + 6H 2 O (1) 4NH 3 + 7O 2 → 4NO 2 + 6H 2 O (2) Number of moles of NH 3 ( g ) is 2.0 0 moles . Number of moles of O 2 ( g ) is 10.0 0 moles . The remaining number of moles of oxygen after the reaction is 6.7 5 moles . Therefore, Number of moles of oxygen reacted is 10.0 0 moles − 6.7 5 moles = 3.2 5 moles The number of moles of oxygen consumed for the reaction (1) is assumed to be x and the number of moles of oxygen consumed for the reaction (2) is assumed to be y . So, the total number of moles of oxygen consumed is. x + y = 3.25 (3) From the reaction (1), 5 moles of O 2 and 4 moles of NH 3 is consumed. For x moles of O 2 , the number of moles of NH 3 consumed is, ( x 5 ) 4 = ( 4 5 ) x . From the reaction (2), 7 moles of O 2 and 4 moles of NH 3 is consumed. For y moles of O 2 , the number of moles of NH 3 consumed is, ( y 7 ) 4 = ( 4 7 ) y . Therefore, the total number of moles of NH 3 consumed is, ( 4 5 ) x + ( 4 7 ) y = 2

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation: The number of moles of NO(g) in the product mixture is calculated.

Concept introduction: The number of moles in an atom is defined as the given mass divided by the molecular mass. One mole is equal to the Avogadro’s number and each element consists of different molar mass that depends on the weight of its atom.

To determine: The number of moles of NO(g) in the product mixture.

Explanation of Solution

Explanation

Given

The balanced chemical reactions are,

4NH3+5O2→4NO+6H2O (1)

4NH3+7O2→4NO2+6H2O (2)

Number of moles of NH3(g) is 2.00 moles .

Number of moles of O2(g) is 10.00 moles .

The remaining number of moles of oxygen after the reaction is 6.75 moles .

Therefore,

Number of moles of oxygen reacted is 10.00 moles−6.75 moles=3.25 moles

The number of moles of oxygen consumed for the reaction (1) is assumed to be x and the number of moles of oxygen consumed for the reaction (2) is assumed to be y .

So, the total number of moles of oxygen consumed is.

x+y=3.25 (3)

From the reaction (1), 5 moles of O2 and 4 moles of NH3 is consumed.

For x moles of O2 , the number of moles of NH3 consumed is,

(x5)4=(45)x .

From the reaction (2), 7 moles of O2 and 4 moles of NH3 is consumed.

For y moles of O2 , the number of moles of NH3 consumed is,

(y7)4=(47)y .

Therefore, the total number of moles of NH3 consumed is,

(45)x+(47)y=2

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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