Test: Ideal Gas Equation - Chemistry MCQ

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.

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.

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.

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.

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.

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.

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.

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.

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.

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.