Gas Laws Test

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Gas Laws Test - 5

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Weekly Quiz Competition

Question 1
1 / -0

What is the relation between volume and pressure of a gas at constant temperature?

A
V P

B

C
V = P

D
P = – V

Solution

The statement of Boyle\'s law is as follows:
Volume of a gas is inversely related to the pressure exerted on it at a given temperature and for a given number of moles.
Question 2
1 / -0

10L of methane gas at 2 atm pressure is compressed to 1.6 l at constant temperature. Which of the following options is the final pressure?

A
6.25 atm

B
12.5 atm

C
0.08 atm

D
0.32 atm

Solution

12.5 atm would be the final pressure.
Question 3
1 / -0

What will be the volume of a gas if its pressure is reduced to half of its initial pressure at constant temperature?

A
Half

B
One-third

C
Double

D
Zero

Solution

If the pressure of the gas is reduced to half of its initial pressure at constant temperature, then the volume of the gas will be doubled.
Question 4
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What is the effect on volume of gas, if pressure is increased in the cylinder?

A
Decreases

B
Increases

C
Remains constant

D
First decreases at maximum and then becomes constant

Solution

According to Boyle's Law, at constant temperature, the volume of a given mass of gas is inversely proportional to its pressure. Hence, if the pressure is increased in the cylinder, the volume decreases.
Question 5
1 / -0

Which of the following graphs represents Boyle's law?

A

B

C

D

Solution

Boyle's law is an experimental gas law which describes how the pressure of a gas tends to decrease as the volume of a gas increases. Thus, according to the definition, the correct graphical representation of Boyle's law is given in option (3).
Question 6
1 / -0

A gas occupies 600 cm³ under 760 mm Hg pressure. At what pressure will the gas occupy 270 cm³ under constant temperature?

A
5.037 mm Hg

B
5.821 cm Hg

C
213.16 mm Hg

D
168.9 cm Hg

Solution

By applying the formula P₁V₁ = P₂V₂, we get
600 760 = P₂ 270
= 600 760 / 270
= 456000 / 270
= 1688.8 mm Hg
= 168.9 cm Hg
Question 7
1 / -0

If pressure is increased by 80%, what would be new volume if the temperature is constant?

A
times of its initial volume

B
times of its initial volume

C
times of its initial volume

D
times of its initial volume

Solution

If the pressure is increased by 80%, the new volume will be times its initial volume at constant temperature.
Question 8
1 / -0

What would be the new volume of a gas if its pressure in a container with capacity 600 ml is decreased by 40%?

A
1000 ml

B
428.57 ml

C
360 ml

D
840 ml

Solution

The new volume of a gas, if its pressure in a container with capacity 600 ml is decreased by 40%, would be 1000 ml.
Question 9
1 / -0

How are volume and temperature related, according to Charles' law?

A

B
V = T

C
V = – T

D

Solution

According to Charles' law, the volume and temperature are related to each other as.
Question 10
1 / -0

What will be the temperature at which the volume of a given mass of gas gets reduced to 3/5^th of original volume at 10° C without any change in pressure.

A
169.8°C

B
– 103.2°C

C
– 169.8 K

D
103.2° C

Solution

Initial condition Final conditionV₁ = V V₂ = 3/5V
T₁ = (273 + 10)K = 283K T₂ = ?
According to Charle\'s Law,
T₂ = V₂
T₂ =
T₂ = 169.8K T₂ = -103.2^oC
Question 11
1 / -0

If V_o is the volume of a gas at 0°C, which of the following options is the correct value of volume of gas at –273°C?

A
0

B
V₀ +

C
V₀

D
V₀ +

Solution

-273^oC or 0 K is called absolute zero, and every gas liquefies before acquiring this temperature.
Considering a hypothetical situation, the volume of the gas would be zero.
Question 12
1 / -0

At what temperature will the volume of a gas at 0°C triple itself if the pressure remains constant?

A
819°C

B
273°C

C
546°C

D
91°C

Solution
Question 13
1 / -0

Which of the following options correctly justifies the bursting of inflated balloon in direct sunlight?

A
The rubber of balloon melts in sunlight.

B
Volume of gas inside the balloon increases.

C
Pressure of gas inside the balloon increases.

D
Sunlight causes holes in the balloon.

Solution

Volume of the gas inside the balloon increases, which correctly justifies the bursting of the inflated balloon in direct sunlight.
Question 14
1 / -0

One mole of a gas occupies a volume of 22.4 litres. This is derived from

A
Berzeliu's hypothesis

B
Gay-Lussac's law

C
Avogadro's law

D
Dalton's law

Solution

Avogadro's law states that under similar conditions of temperature and pressure, equal moles will occupy equal molecules. Actually, 1 mole of any gas at standard conditions (0^oC, 1 atm pressure) is found to occupy a volume of 22.4 litres. This volume is known as standard molar volume.
Question 15
1 / -0

What would be the effect on pressure if both volume and temperature of a gas are doubled?

A
Double

B
Half

C
Quadruple

D
Remain same

Solution

If both volume and temperature of a gas are doubled, the pressure will remain the same.
Question 16
1 / -0

Which of the following expressions represents gas equation?

A

B

C
PV = nRT

D
P₁V₁ = P₂V₂

Solution

The expression for gas equation is as follows:
=
Question 17
1 / -0

How is kinetic energy related to absolute temperature?

A
K.E. Absolute temperature

B
K.E.

C
K.E. = – Absolute temperature

D
K.E. is not related to absolute temperature

Solution

Kinetic energy is directly proportional to absolute temperature.
Question 18
1 / -0

Which of the following options is not in accordance with kinetic molecular theory of gases?

A
A gas is composed of large number of molecules.

B
Gases have large intermolecular spaces between their molecules.

C
The molecules of gas lose kinetic energy on collision.

D
Kinetic energy of the molecules of gas increases with increase in temperature.

Solution

According to kinetic molecular theory of gases, molecules do not lose any kinetic energy when they collide with one another.
Question 19
1 / -0

What are the values of standard temperature and pressure of a gas?

A
0°C and 760 mm Hg

B
0 K and 1 atm

C
273 K and 760 atm

D
0°C and 760 atm

Solution

The respective values of standard temperature and pressure of a gas are 0°C and 760 mm Hg.
Question 20
1 / -0

What is the relationship between Celsius and Kelvin scales of temperature?

A
K = °C + 273

B
K = °C – 273

C
K = °C + 1/273

D
K = °C 273

Solution

The correct relationship between Celsius and Kelvin scales of temperature is K = °C + 273.