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Derivation of Ideal Gas Equation MCQ - Practice Questions with Answers

Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

Quick Facts

Ideal Gas Equation is considered one of the most asked concept.
2 Questions around this concept.

Solve by difficulty

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of 1 atm but also a concentration of 1 mol litre^-1. [ R = 0.082 litre atm mol^-1 K^-1 ]

at S.T.P

when V = 22.42 L

when T = 12 K

Impossible under any condition

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Ideal Gas Equation

Ideal Gas Equation
Ideal gas equation is an equation which is followed by the ideal gases. A gas that would obey Boyle's and Charles Law under all the conditions of temperature and pressure is called an ideal gas.
As discussed the behaviour of gases is described by certain laws as Avogadro's Law, Boyle's Law, Charles' Law.

$\begin{array}{l}{\text { According to Avogadro's Law ; } \mathrm{V} \propto \mathrm{n}(\mathrm{P} \text { and } \mathrm{T} \text { constant) }} \\ {\text { According to Boyle's Law ; } \mathrm{V} \propto \frac{1}{P}(\mathrm{T} \text { and n constant) }} \\ {\text { According to Charles' Law; } \mathrm{V} \propto \mathrm{T}(\mathrm{P} \text { and n constant) }} \\ {\text { Combining the three laws; we get: }}\end{array}$

$\begin{array}{l}{V \propto \frac{n T}{P}} \\\\ {V=R \frac{n T}{P}}\end{array}$

$\begin{array}{l}{\text { 'R' is the proportionality constant. On rearranging the above equation we get: }} \\ {\text { PV = nRT }} \\ {\text { This is the ideal gas equation as it is obeyed by the hypothetical gases called ideal gases under all conditions }}\end{array}$

Universal Gas Constant or Ideal Gas Constant
$\begin{array}{l}{\text { Ror S: Molar gas constant or universal gas constant }} \\ {\text { Values of } \mathrm{R}=0.0821 \text { lit, atm, } \mathrm{K}^{-1}, \mathrm{mol}^{-1}} \\ {\qquad \begin{array}{l}{=8.314 \text { joule } \mathrm{K}^{-1} \mathrm{mol}^{-1}} \\ {=8.314 \times 10^{7} \operatorname{erg} \mathrm{K}^{-1} \mathrm{mol}^{-1}} \\ {=2 \mathrm{\, cal} \mathrm{\, K}^{-1} \mathrm{\, mol}^{-1}}\end{array}}\end{array}$

$\begin{array}{l}{\text {For a single molecule, gas constant is known as }} \\ {\text {Boltzmann constant }(\mathrm{k}) \text { . }} \\ {\mathrm{k}=\mathrm{R} \mathrm{N}_{0}} \\ {\: \: \: \, =1.38 \times 10^{-3} \mathrm{J} / \mathrm{deg-abs} / \mathrm{molecule}} \\ {\: \: \: \, =1.38 \times 10^{-16} \text { erg/deg-abs/molecule }}\end{array}$

Combined gas law:
The Boyle's and Charles' Law can be combined to give a relationship between the three variables P, V and T. The initial temperature, pressure and volume of a gas are . With the change in either of the variables, all the three variables change to . Then we can write:

Combining the both above equation we get

The above relation is called the combined gas law.

Density and Molar Mass of a Gaseous Substance

$\\\mathrm{Ideal \: gas\: equation\: is \: PV = nRT \quad \quad \quad.......(i)}\\\mathrm{\text {On rearranging the above equation, we get }}\\\\\mathrm{\frac{\mathrm{n}}{\mathrm{V}}=\frac{\mathrm{P}}{\mathrm{RT}}\quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad\: \: \: .......(ii)}\\\\\mathrm{n\left(N_{0} . \text { of moles }\right)=\frac{\text { Given mass }(m)}{\text { Molar mass }(M)}\quad....(iii)}\\\\\text {Putting the value of 'n' from equation (iii) in equation (ii), we get: }\\\\\frac{\mathrm{m}}{\mathrm{MV}}=\frac{\mathrm{P}}{\mathrm{RT}}\quad \quad \quad \quad \quad \quad \quad \quad \quad\quad\quad\: \: \: \: .........(iv)\\\\\text {We know that density (d) is mass (m) per unit volume (V) }\\\\\mathrm{d}=\frac{\mathrm{m}}{\mathrm{V}}\quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad \quad .........(v)\\\\\text {Replacing } \frac{\mathrm{m}}{\mathrm{V}} \text { in eq. (iv) with d(density), then equation (iv) becomes:}\\\\$