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

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

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

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

2 / 39

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

A) Density of gas

B) Number of atoms only

C) Number of molecules

D) Amount of substance in moles

3 / 39

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

A) Avogadro’s number

B) Number of molecules

C) Number of atoms per mole

D) Number of moles

4 / 39

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

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

B) bar

C) $\mathbf{mmHg}$

D) $\mathbf{atm}$

5 / 39

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

A) Milliliter

B) Cubic centimeter

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

D) Liter

6 / 39

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

A) Double

B) Quadruple

C) Halve

D) Remain constant

7 / 39

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

A) Mass

B) Temperature

C) Volume

D) Density

8 / 39

Temperature in the ideal gas equation must be measured in:

A) Kelvin

B) Celsius

C) Centigrade

D) Fahrenheit

9 / 39

Which quantity remains constant for a fixed sample of gas?

A) Volume

B) Pressure

C) Temperature

D) Number of moles

10 / 39

If volume decreases while temperature remains constant, pressure:

A) Remains unchanged

B) Decreases

C) Increases

D) Becomes zero

11 / 39

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

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

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

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

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

12 / 39

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

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

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

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

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

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

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

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

14 / 39

One mole of any ideal gas contains:

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

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

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

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

15 / 39

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

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

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

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

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

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

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

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

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

17 / 39

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

A) Doubles

B) Halves

C) Remains constant

D) Becomes zero

18 / 39

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

A) Temperature

B) Volume

C) Number of moles

D) Pressure

19 / 39

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

A) Double

B) Half

C) Four times

D) Unchanged

20 / 39

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

A) Density only

B) Mass only

C) Volume only

D) Number of molecules and temperature

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) $\mathbf{300000\ J}$

B) $\mathbf{300\ J}$

C) $\mathbf{30000\ J}$

D) $\mathbf{3000\ J}$

22 / 39

Which assumption is made for an ideal gas?

A) Molecules occupy large volume

B) Molecules attract strongly

C) Intermolecular forces are negligible

D) Molecules are stationary

23 / 39

If temperature decreases while volume remains constant, pressure:

A) Becomes infinite

B) Decreases

C) Increases

D) Remains constant

24 / 39

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

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

B) $\mathbf{P}$ vs density

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

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

25 / 39

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

A) Number of moles only

B) Volume only

C) Temperature only

D) $\mathbf{(nT)}$

26 / 39

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

A) Becomes zero

B) Halves

C) Remains unchanged

D) Doubles

27 / 39

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

A) Amount of gas representation

B) Volume

C) Pressure

D) Temperature

28 / 39

Why is Kelvin scale used in gas equations?

A) It avoids negative temperatures in gas laws.

B) It gives direct proportionality with molecular kinetic energy.

C) All of the above

D) It starts at absolute zero.

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

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

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

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

30 / 39

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

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

B) Density

C) Pressure only

D) Volume only

31 / 39

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

A) Number of molecules

B) Density

C) Mass only

D) Pressure

32 / 39

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

A) Charles’s law

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

C) Hooke’s law

D) Boyle’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) Half

C) Four times

D) Same

34 / 39

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

A) Number of moles

B) Density only

C) Pressure again

D) Molecular mass only

35 / 39

The ideal gas equation combines:

A) Laws of motion and gravitation

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

C) Newton’s laws

D) Hooke’s and Boyle’s 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) $\mathbf{0.25\ m}^{\mathbf{3}}$

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

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

37 / 39

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

A) Doubles

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

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

D) Remains constant

38 / 39

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

A) Pressure

B) Temperature

C) Volume

D) Number of moles

39 / 39

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

A) Connects macroscopic gas behavior with molecular quantities

B) Applies only to liquids

C) Eliminates temperature

D) Ignores molecules

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