This set of Class 11 Chemistry Chapter 5 Multiple Choice Questions & Answers (MCQs) focuses on “States of Matter – Ideal Gas Equation”.

1. What is the constant in ideal gas equation known as?

a) Universal gas constant

b) Pressure constant

c) Temperature constant

d) Boltzmann constant

View Answer

Explanation: The ideal gas equation is given by PV = nRT where P is pressure, V is volume, n is the number of moles, T is the temperature in Kelvin and R is given by universal gas constant its value is 8.314kgm

^{2}s

^{-2}.

2. A certain gas occupies 200 ml of volume at 2 bar pressure at hundred degrees Kelvin. How much volume does it occupy at 5 bar pressure and 200 degrees Kelvin?

a) 200 ml

b) 160 ml

c) 240 ml

d) 320 ml

View Answer

Explanation: From ideal gas law, we know that P

_{1}V

_{1}/T

_{1}= P

_{2}V

_{2}/T

_{2}. Here we take P

_{1}as 2 bar, V

_{1}as 200 ml, T

_{1}as hundred degrees Kelvin, P

_{2}as 5 bar and T

_{2}as 200 degrees Kelvin, so by substituting the above values 200 x 2/100 = 5 x V

_{2}/200; V

_{2}= 160 ml.

3. Which of the following do you think is a correct relationship between the molar mass of gas temperature and its pressure?

a) M = dRT/P

b) M = dRT/V

c) PV = nRT

d) M = VRT/P

View Answer

Explanation: We know that the ideal gas equation is given by PV = nRT. Number of moles = n; can also be written as m/M, so PV = nRT becomes, PV = mRT/M. We also have density d = m/V, so molar mass M = dRT/P.

4. If the pressure of dry gas is given by X and the total pressure is given by X + 3, then what is aqueous tension?

a) 2

b) X

c) X + 2

d) 3

View Answer

Explanation: As we know that the pressure of the dry gas is given by the difference between the total pressure and the Aqueous tension, so aqueous tension equals x + 3 – x = 3. So the aqueous tension is three units.

5. In a cylinder of pressure 1 bar, there is the hydrogen of 20 grams and neon of 50 grams, what is a partial pressure of hydrogen?

a) 0.2

b) 0.8

c) 0.4

d) 0.6

View Answer

Explanation: As we know that the partial pressure of a gas is the product of its mole fraction and the total pressure of the gases present, so here the partial pressure of hydrogen is 10/10 + 2.5 = 0.8. Mole fraction is given by the number of moles of required as per the total number of the gas moles.

6. If the partial pressure of oxygen is given by three bar and the partial pressure of the other gas is four bar, then what is a total pressure that is exerted?

a) 7 bar

b) 3 bar

c) 4 bar

d) 1 bar

View Answer

Explanation: The total pressure that is exerted is given by the sum of the partial pressure of the gases present. By adding, the sum of the partial pressures is 3bar + 4bar = 7bar, so the total pressure is 7 bar in this case.

7. Who gave the law regarding the partial pressure?

a) Charles

b) Dalton

c) Lussac

d) Thomas

View Answer

Explanation: Dalton proposed law regarding the partial pressures, that the total pressure that is exerted by non-reactive gases is the sum of the individual gas’s partial pressures. P

_{tot}= ∑P

_{i}, i = 1, 2, 3, 4, … n.

8. The partial pressure of a gas X is given by two bar, where is the total pressure of the gaseous mixture in a cylinder is 10 bar. What is the mole fraction of the gas X in that mixture?

a) 0.5

b) 2

c) 0.2

d) 5

View Answer

Explanation: The partial pressure of a gas equals the mole fraction of the gas in the gaseous mixture x the total pressure that is exerted by the gaseous mixture. So here 2 bar = molar fraction x 10 bar, we get that the mole fraction is 2/10 = 0.2.

9. In a balloon of total pressure 6 atm there is a gaseous composition of 44 grams of carbon dioxide 16 grams of by oxygen and 7 grams of nitrogen, what is the ratio of nitrogen partial pressure do the total pressure in the balloon?

a) 0.25

b) 0.5

c) 0.75

d) 1

View Answer

Explanation: The partial pressure of a gas is given by the mole fraction of the gas x the total pressure, so the ratio of the partial pressure to the total pressure is the mole fraction of nitrogen is 7/14 divided by 44/44 + 16/32 2 + 7/14 = 0.25.

10. Consider a gas of n moles at a pressure of P and a temperature of T in Celsius, what would be its volume?

a) nR(T + 273)/p

b) nRT/p

c) nR(T – 273)/p

d) R(T + 273)/p

View Answer

Explanation: The ideal gas equation is given NY PV = not where p is pressure is the volume and is the number of moles are is universal gas constant and T is a temperature in Kelvin. So by arranging, we V = nR(T + 273)/p, as T is in Celcius, we need to add 273.

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