a. nR/P b. nR/P2 c. 1/T d. 1/P e. 1/V 6) At 25 °C and 1 bar, the mass density of
ID: 1660724 • Letter: A
Question
a. nR/P b. nR/P2 c. 1/T d. 1/P e. 1/V 6) At 25 °C and 1 bar, the mass density of N2 gas is 1.129 kg m-3. Assume N2 gas behaves as perfect gas. Validate the molecular weight of N2 is ~28 g mol1? Dalton's law 7) In the reaction of reducing CO2 to CO with H2, a vessel of volume 25 dm3 contains 1 mol CO2 and 2 mol H2 at 25 °C initially. Calculate the partial pressures and the total pressure of the mixture. The Kinetic model 8) Given the kinetic model of idea gas PV = -, where M is the molecular weight and c the average velocity of gas molecules, justify the kinetic energy of gas molecules is dependent on temperature only (for ideal gas). Real gas nMc2 MExplanation / Answer
6)
P= 1.0 bar
= (1.0/1.01325) atm
= 0.9869 atm
T= 25.0 oC
= (25.0+273) K
= 298 K
density = 1.129 kg/m^3 = 1.129 g/L
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T
Put Values:
0.9869 atm * MM = 1.129g/L * 0.08206 atm.L/mol.K *298.0 K
MM = 28 g/mol
Answer: 28 g/mol
I am allowed to answer only 1 question at a time
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.