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Test: Ideal Gas Equation - Chemistry MCQ


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10 Questions MCQ Test Physical Chemistry - Test: Ideal Gas Equation

Test: Ideal Gas Equation for Chemistry 2024 is part of Physical Chemistry preparation. The Test: Ideal Gas Equation questions and answers have been prepared according to the Chemistry exam syllabus.The Test: Ideal Gas Equation MCQs are made for Chemistry 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Test: Ideal Gas Equation below.
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Test: Ideal Gas Equation - Question 1

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?

Detailed Solution for Test: Ideal Gas Equation - Question 1

From ideal gas law, we know that P1V1/T1 = P2V2/T2. Here we take P1 as 2 bar, V1 as 200 ml, T1 as hundred degrees Kelvin, P2 as 5 bar and T2 as 200 degrees Kelvin, so by substituting the above values 200 x 2/100 = 5 x V2/200; V2 = 160 ml.

Test: Ideal Gas Equation - Question 2

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

Detailed Solution for Test: Ideal Gas Equation - Question 2

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.

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Test: Ideal Gas Equation - Question 3

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?

Detailed Solution for Test: Ideal Gas Equation - Question 3

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.

Test: Ideal Gas Equation - Question 4

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?

Detailed Solution for Test: Ideal Gas Equation - Question 4

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.

Test: Ideal Gas Equation - Question 5

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

Detailed Solution for Test: Ideal Gas Equation - Question 5

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.

Test: Ideal Gas Equation - Question 6

What is the constant in ideal gas equation known as?

Detailed Solution for Test: Ideal Gas Equation - Question 6

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 8.314kgm2s-2.

Test: Ideal Gas Equation - Question 7

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

Detailed Solution for Test: Ideal Gas Equation - Question 7

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.

Test: Ideal Gas Equation - Question 8

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?

Detailed Solution for Test: Ideal Gas Equation - Question 8

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.

Test: Ideal Gas Equation - Question 9

Who gave the law regarding the partial pressure?

Detailed Solution for Test: Ideal Gas Equation - Question 9

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. Ptot = ∑Pi , i = 1, 2, 3, 4, … n.

Test: Ideal Gas Equation - Question 10

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?

Detailed Solution for Test: Ideal Gas Equation - Question 10

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.

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