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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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Consider the following reaction: 4 NH 3 ( g ) + 5 O 2 ( g ) 4 NO ( g ) + 6 H 2 O ( g )

a container were to have only 10 molecules of O 2 ( g ) and 10 molecules of NH 3 ( g ) , how many total molecules (reactant and product) would be present in the container after the above reaction goes to completion?

ing “microscopic” pictures, draw the total molecules present inside the container after the reaction occurs.

at mass of NO ( g ) is present in the container after the reaction occurs? (Report your final answer to 4 significant figures.)

Interpretation Introduction

(a)

Interpretation:

The total number of the molecules present in the system after 10 molecules of NH3 and 10 molecules of O2 take part in the complete reaction should be calculated.

Concept Introduction:

It is important to recognize that the coefficients in a balanced equation give the relative number of molecules.

Because atoms are not changed or destroyed in a chemical reaction one must always balance a chemical reaction. That is, one must choose the coefficients that gives the same number of each type of atoms on both sides, using the smallest set of integers.

If the stoichiometric quantities of two reactants is not same in a reaction, it is important to determine the limiting and excess reactant to calculate the correct amount (in mass) of products formed.

Explanation

The balanced chemical reaction is as follows:

4NH3(g) + 5O2(g)4NO(g) + 6H2O(l)

According to the stoichiometry 5 mol of O2 gas reacts with 4 mol of NH3(g).

Since,

1 mol= 6.022×1023 mol 

One can also say,

5 molecules of O2(g) reacts with 4 molecules of  NH3(g)

Therefore, according to stoichiometry,

Number of NH3(g) molecules required to react with 10 molecules of O2(g) can be calculated as follows:

no of NH3(g) molecules required to react with 10 molecules of O2(g)

=  4 molecules of  NH3(g) 5 molecules of O2(g)× 10 molecules of O2(g) = 8 molecules of NH3(g)

The number of molecules of ammonia are 10 thus, it is present in excess and oxygen is limiting reactant

Interpretation Introduction

(b)

Interpretation:

Making use of the microscopic pictures, the total molecules present inside the container after the reaction occurs should be determined.

Concept Introduction:

It is important to recognize that the coefficients in a balanced equation give the relative number of molecules.

Because atoms are not changed or destroyed in a chemical reaction one must always balance a chemical reaction. That is, one must choose the coefficients that gives the same number of each type of atoms on both sides, using the smallest set of integers.

If the stoichiometric quantities of two reactants is not same in a reaction, it is important to determine the limiting and excess reactant to calculate the correct amount (in mass) of products formed.

Interpretation Introduction

(c)

Interpretation:

The mass of NO(g) in grams present in the container after the reaction occurs should be calculated.

Concept Introduction:

It is important to recognize that the coefficients in a balanced equation give the relative number of molecules.

Because atoms are not changed or destroyed in a chemical reaction one must always balance a chemical reaction. That is, one must choose the coefficients that gives the same number of each type of atoms on both sides, using the smallest set of integers.

If the reactants are not mixed in stoichiometric quantities in any stoichiometry problem, it is important to determine the limiting reactant to calculate the correct amount of product formed in the reaction. This reagent which is celled the limiting reactant is an essential factor in determining the number of products formed or reactants used whenever reactants are not mixed in stoichiometric quantities.

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