A gas contains a mixture of NH 3 ( g ) and N 2 H 4 ( g ), both of which react with O 2 ( g ) to form NO 2 ( g ) and H 2 O( g ). The gaseous mixture (with an initial mass of 61.00 g) is reacted with 10.00 moles O 2 , and after the reaction is complete, 4.062 moles of O 2 remains. Calculate the mass percent of N 2 H 4 ( g ) in the original gaseous mixture.

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Interpretation Introduction Interpretation: The mass percent of N 2 H 4 ( g ) in the original gaseous mixture is to be calculated. Concept introduction: Mass percent of an element is defined as the ratio of mass of the element divided by the total mass of the compound. The number of moles is defined as the ratio of mass with the molecular mass of an element. The mass of an element is the amount of the substance present in an element. To determine: The mass percent of N 2 H 4 ( g ) in the original gaseous mixture. Explanation Explanation Given The mass of gaseous mixture is 61. 00 g . The number of moles of O 2 10 .00 moles . The number of moles of O 2 remained after the reaction is 4.06 2 moles . The given reaction is, 4NH 3 + 7 O 2 → 4 NO 2 + 6H 2 O (1) N 2 H 4 + 3 O 2 → 2NO 2 + 2 H 2 O (2) The overall reaction is, 4NH 3 + N 2 H 4 + 10 O 2 → 6NO 2 + 8 H 2 O (3) The number of moles of O 2 first consumed in the reaction is calculated as, Moles of O 2 consumed = Total moles of O 2 − Moles of O 2 remained . Substitute the value of total and remained moles of O 2 in the above expression to calculate the number of moles of O 2 consumed. Moles of O 2 consumed = Total moles of O 2 − Moles of O 2 remained = 10.0 0 mol − 4.06 2 mol = 5.93 8 mol Now observing the reaction it is found that total parts of oxygen are required. So moles of oxygen required for N 2 H 4 = 5.938 × 3 10 = 1.7 8 mol So the moles of N 2 H 4 is one third moles of O 2 in the second reaction. It is calculated as, Moles of N 2 H 4 = 1 3 Moles of O 2 Substitute the value of moles of O 2 required for N 2 H 4 in the above expression to calculate the moles of N 2 H 4

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

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Interpretation Introduction

Interpretation: The mass percent of N2H4(g) in the original gaseous mixture is to be calculated.

Concept introduction: Mass percent of an element is defined as the ratio of mass of the element divided by the total mass of the compound. The number of moles is defined as the ratio of mass with the molecular mass of an element. The mass of an element is the amount of the substance present in an element.

To determine: The mass percent of N2H4(g) in the original gaseous mixture.

Explanation of Solution

Explanation

Given

The mass of gaseous mixture is 61.00 g .

The number of moles of O2 10.00 moles .

The number of moles of O2 remained after the reaction is 4.062 moles .

The given reaction is,

4NH3+7O2→4NO2+6H2O (1)

N2H4+3O2→2NO2+2H2O (2)

The overall reaction is,

4NH3+N2H4+10O2→6NO2+8H2O (3)

The number of moles of O2 first consumed in the reaction is calculated as,

Moles of O2 consumed=Total moles of O2−Moles of O2 remained .

Substitute the value of total and remained moles of O2 in the above expression to calculate the number of moles of O2 consumed.

Moles of O2 consumed=Total moles of O2−Moles of O2 remained=10.00 mol−4.062 mol=5.938 mol

Now observing the reaction it is found that total parts of oxygen are required. So moles of oxygen required for N2H4 =5.938×310=1.78 mol

So the moles of N2H4 is one third moles of O2 in the second reaction. It is calculated as,

Moles of N2H4=13Moles of O2

Substitute the value of moles of O2 required for N2H4 in the above expression to calculate the moles of N2H4

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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