Physics 11th Chap 8 : Topic 3 - Maryam Publications

Physics Chapter 8 : Topic 3

Ideal Gas Equation

1 / 39

The equation of state for an ideal gas is:

A) $\mathbf{(P\ /\ T = nRV)}$

B) $\mathbf{(PV = RT\ /\ n)}$

C) $\mathbf{(PV = nR\ /\ T)}$

D) $\mathbf{(PV = nRT)}$

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In the equation $\mathbf{(PV = nRT)}$, the symbol $\mathbf{(n)}$ represents:

A) Number of molecules

B) Density of gas

C) Amount of substance in moles

D) Number of atoms only

3 / 39

In the equation $\mathbf{(PV = NkT)}$, the symbol $\mathbf{(N)}$ represents:

A) Number of moles

B) Avogadro’s number

C) Number of molecules

D) Number of atoms per mole

4 / 39

The SI unit of pressure used in the ideal gas equation is:

A) $\mathbf{atm}$

B) $\mathbf{mmHg}$

C) Pascal $\mathbf{(Pa)}$

D) bar

5 / 39

The SI unit of volume in $\mathbf{(PV = nRT)}$ is:

A) Milliliter

B) Cubic meter $\mathbf{(}\mathbf{m}^{\mathbf{3}}\mathbf{)}$

C) Cubic centimeter

D) Liter

6 / 39

If the temperature of an ideal gas doubles while pressure remains constant, the volume will:

A) Quadruple

B) Halve

C) Remain constant

D) Double

7 / 39

For a fixed amount of gas at constant temperature, pressure is inversely proportional to:

A) Temperature

B) Density

C) Volume

D) Mass

8 / 39

Temperature in the ideal gas equation must be measured in:

A) Kelvin

B) Celsius

C) Fahrenheit

D) Centigrade

9 / 39

Which quantity remains constant for a fixed sample of gas?

A) Number of moles

B) Temperature

C) Pressure

D) Volume

10 / 39

If volume decreases while temperature remains constant, pressure:

A) Remains unchanged

B) Becomes zero

C) Increases

D) Decreases

11 / 39

The gas constant $\mathbf{(R)}$ has a value approximately equal to:

A) $\mathbf{9.8\ N\ /\ kg}$

B) $\mathbf{1.38 \times}\mathbf{10}^{\mathbf{- 23}}\mathbf{\ J\ /\ K}$

C) $\mathbf{6.02 \times}\mathbf{10}^{\mathbf{23}}$

D) $\mathbf{8.31\ }\mathbf{J\ mol}^{\mathbf{- 1\ }}\mathbf{K}^{\mathbf{- 1}}$

12 / 39

The Boltzmann constant $\mathbf{(k)}$ is approximately:

A) $\mathbf{6.67 \times}\mathbf{10}^{\mathbf{- 11}}$

B) $\mathbf{1.38 \times}\mathbf{10}^{\mathbf{- 23}}\mathbf{\ J\ K}^{\mathbf{- 1}}$

C) $\mathbf{8.31\ }\mathbf{J\ mol}^{\mathbf{- 1\ }}\mathbf{K}^{\mathbf{- 1}}$

D) $\mathbf{1.6 \times}\mathbf{10}^{\mathbf{- 19}}\mathbf{\ J}$

13 / 39

Which equation relates pressure and volume directly to the number of molecules?

A) $\mathbf{(PV = nRT)}$

B) $\mathbf{(P = nRT)}$

C) $\mathbf{(PV = NkT)}$

D) $\mathbf{(PV = RT)}$

14 / 39

One mole of any ideal gas contains:

A) $\mathbf{1.38 \times}\mathbf{10}^{\mathbf{- 23}}$ molecules

B) $\mathbf{9.8 \times}\mathbf{10}^{\mathbf{23}}$ molecules

C) $\mathbf{6.02 \times}\mathbf{10}^{\mathbf{23}}$ molecules

D) $\mathbf{8.31 \times}\mathbf{10}^{\mathbf{23}}$ molecules

15 / 39

The relationship between $\mathbf{(R)}$ and $\mathbf{(k)}$ is:

A) $\mathbf{R =}\mathbf{N}_{\mathbf{A}}\mathbf{\ /\ k}$

B) $\mathbf{R =}\mathbf{N}_{\mathbf{A}}\mathbf{\ k}$

C) $\mathbf{k =}\mathbf{R\ N}_{\mathbf{A}}$

D) $\mathbf{R =}\mathbf{k\ /\ N}_{\mathbf{A}}$

16 / 39

An ideal gas occupies $\mathbf{2\ m}^{\mathbf{3}}$ at pressure $\mathbf{2 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ Pa}$. The product $\mathbf{(PV)}$ is:

A) $\mathbf{1 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ J}$

B) $\mathbf{4 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ J}$

C) $\mathbf{2 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ J}$

D) $\mathbf{8 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ J}$

17 / 39

If the number of moles is doubled while $\mathbf{(P)}$ and $\mathbf{(T)}$ remain constant, the volume:

A) Becomes zero

B) Halves

C) Remains constant

D) Doubles

18 / 39

Which variable must never be expressed in Celsius in gas law calculations?

A) Temperature

B) Number of moles

C) Pressure

D) Volume

19 / 39

A gas at $\mathbf{300\ K}$ is heated to $\mathbf{600\ K}$ at constant volume. The pressure becomes:

A) Unchanged

B) Four times

C) Half

D) Double

20 / 39

The equation $\mathbf{(PV = NkT)}$ shows that pressure depends directly on:

A) Number of molecules and temperature

B) Density only

C) Mass only

D) Volume only

21 / 39

An ideal gas has pressure $\mathbf{1 \times}\mathbf{10}^{\mathbf{5}}\mathbf{\ Pa}$ and volume $\mathbf{0.03\ m}^{\mathbf{3}}$. Calculate $\mathbf{(PV)}$.

A) $\mathbf{3000\ J}$

B) $\mathbf{300\ J}$

C) $\mathbf{30000\ J}$

D) $\mathbf{300000\ J}$

22 / 39

Which assumption is made for an ideal gas?

A) Intermolecular forces are negligible

B) Molecules are stationary

C) Molecules attract strongly

D) Molecules occupy large volume

23 / 39

If temperature decreases while volume remains constant, pressure:

A) Remains constant

B) Increases

C) Decreases

D) Becomes infinite

24 / 39

Which graph is a straight line for an ideal gas at constant pressure?

A) $\mathbf{P}$ vs density

B) $\mathbf{P}$ vs $\mathbf{V}$

C) $\mathbf{P}$ vs $\mathbf{1/V}$

D) $\mathbf{V}$ vs $\mathbf{T(K)}$

25 / 39

The product $\mathbf{(PV)}$ for an ideal gas is proportional to:

A) $\mathbf{(nT)}$

B) Volume only

C) Temperature only

D) Number of moles only

26 / 39

If the number of molecules doubles at constant volume and temperature, pressure:

A) Remains unchanged

B) Halves

C) Doubles

D) Becomes zero

27 / 39

Which quantity distinguishes $\mathbf{(PV = nRT)}$ from $\mathbf{(PV = NkT)}$?

A) Temperature

B) Pressure

C) Amount of gas representation

D) Volume

28 / 39

Why is Kelvin scale used in gas equations?

A) All of the above

B) It starts at absolute zero.

C) It gives direct proportionality with molecular kinetic energy.

D) It avoids negative temperatures in gas laws.

29 / 39

A gas occupies $\mathbf{1\ m}^{\mathbf{3}}$ at $\mathbf{300\ K}$. At constant pressure, its volume at $\mathbf{600\ K}$ is:

A) $\mathbf{0.5\ m}^{\mathbf{3}}$

B) $\mathbf{1\ m}^{\mathbf{3}}$

C) $\mathbf{2\ m}^{\mathbf{3}}$

D) $\mathbf{4\ m}^{\mathbf{3}}$

30 / 39

The quantity $\mathbf{(NkT)}$ represents:

A) Pressure only

B) Density

C) Product $\mathbf{(PV)}$

D) Volume only

31 / 39

If pressure and temperature are constant, volume is directly proportional to:

A) Number of molecules

B) Density

C) Pressure

D) Mass only

32 / 39

Which law can be derived from $\mathbf{(PV = nRT)}$ when volume is constant?

A) Pressure law $\mathbf{(P \propto T)}$

B) Hooke’s law

C) Boyle’s law

D) Charles’s law

33 / 39

A gas sample contains twice as many molecules as another sample at the same temperature and volume. Its pressure is:

A) Double

B) Four times

C) Same

D) Half

34 / 39

In $\mathbf{PV = nRT}$, if $\mathbf{P}$, $\mathbf{V}$, and $\mathbf{T}$ are known, one can determine:

A) Density only

B) Number of moles

C) Molecular mass only

D) Pressure again

35 / 39

The ideal gas equation combines:

A) Newton’s laws

B) Laws of motion and gravitation

C) Hooke’s and Boyle’s laws

D) Boyle’s, Charles’s and Pressure laws

36 / 39

A gas occupies $\mathbf{0.5\ m}^{\mathbf{3}}$ at $\mathbf{200\ K}$. At constant pressure, what is its volume at $\mathbf{400\ K}$?

A) $\mathbf{2.0\ m}^{\mathbf{3}}$

B) $\mathbf{0.5\ m}^{\mathbf{3}}$

C) $\mathbf{0.25\ m}^{\mathbf{3}}$

D) $\mathbf{1.0\ m}^{\mathbf{3}}$

37 / 39

If temperature increases by $\mathbf{50\%}$ at constant volume, pressure:

A) Doubles

B) Remains constant

C) Increases by $\mathbf{50\%}$

D) Decreases by $\mathbf{50\%}$

38 / 39

Which quantity remains unchanged in the equation $\mathbf{(PV = nRT)}$ for a sealed container?

A) Number of moles

B) Volume

C) Temperature

D) Pressure

39 / 39

The equation $\mathbf{(PV = NkT)}$ is particularly useful because it:

A) Ignores molecules

B) Connects macroscopic gas behavior with molecular quantities

C) Applies only to liquids

D) Eliminates temperature

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