Chapter 6, Problem 6.36AP

(a)

Interpretation Introduction

Interpretation:

The balanced equation should be determined for the reaction of $N_2$ with $O_2$ and results to yield $NO$.

Concept introduction:

Chemical equation is the representation of a chemical reaction, in which the reactants and products of the reactions are represented left and right side of an arrow respectively by using their respective chemical formulas.

Reactant of a chemical reaction is the substrate compounds or the compounds which undergo a chemical reaction.

Product of a chemical reaction is the produced compounds or the compounds formed after a chemical reaction.

Balanced chemical equation of a reaction is written according to law of conservation of mass.

(b)

Interpretation Introduction

Interpretation:

The number of moles of ${\text{N}}_{\text{2}}$ required to react with $7.50molof{O}_2$ should be calculated.

Concept introduction:

Mass: It is the quantitative measure of a substance. The amount of matter present in substance is expressed as mass. The $S.I.$ unit of mass is $kg$.

Moles: One mole is equivalent to the mass of the substance consists same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

From given mass of substance moles could be calculated by using the following formula,

$\text{Moles}\text{of}\text{substance}\left(mol\right)\text{= }\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Molar}\text{mass}\left(\text{g/mol}\right)}$

Molar mass: It is obtained by dividing the mass of substance with the amount of substance and the S.I. unit of molar mass is $\text{kg/mol}$. It is numerically equal to the molecular weight since molecular weight is sum of all individual atom weight present in molecule which is represented in $amu$.

$\text{Molar}\text{mass}\left(\text{g/mol}\right)=\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Moles}\text{of}\text{substance}\left(mol\right)}$

(c)

Interpretation Introduction

Interpretation:

The moles of $NO$ formed when $3.81molof{N}_2$ reacts should be determined.

Concept introduction:

Mass: It is the quantitative measure of a substance. The amount of matter present in substance is expressed as mass. The $S.I.$ unit of mass is $kg$.

Moles: One mole is equivalent to the mass of the substance consists same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

From given mass of substance moles could be calculated by using the following formula,

$\text{Moles}\text{of}\text{substance}\left(mol\right)\text{= }\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Molar}\text{mass}\left(\text{g/mol}\right)}$

Molar mass: It is obtained by dividing the mass of substance with the amount of substance and the S.I. unit of molar mass is $\text{kg/mol}$. It is numerically equal to the molecular weight since molecular weight is sum of all individual atom weight present in molecule which is represented in $amu$.

$\text{Molar}\text{mass}\left(\text{g/mol}\right)=\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Moles}\text{of}\text{substance}\left(mol\right)}$

(d)

Interpretation Introduction

Interpretation:

The moles of $O_2$ required for production of $\text{0}\text{.250}\text{mol of NO}$ should be determined.

Concept introduction:

Mass: It is the quantitative measure of a substance. The amount of matter present in substance is expressed as mass. The $S.I.$ unit of mass is $kg$.

Moles: One mole is equivalent to the mass of the substance consists same number of units equal to the atoms present in $\text{12}\text{g}$ of ${}^{\text{12}}\text{C}$.

From given mass of substance moles could be calculated by using the following formula,

$\text{Moles}\text{of}\text{substance}\left(mol\right)\text{= }\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Molar}\text{mass}\left(\text{g/mol}\right)}$

Molar mass: It is obtained by dividing the mass of substance with the amount of substance and the S.I. unit of molar mass is $\text{kg/mol}$. It is numerically equal to the molecular weight since molecular weight is sum of all individual atom weight present in molecule which is represented in $amu$.

$\text{Molar}\text{mass}\left(\text{g/mol}\right)=\frac{\text{Given}\text{mass}\text{of}\text{substance}\left(\text{g}\right)}{\text{Moles}\text{of}\text{substance}\left(mol\right)}$