Question

1. Consider three, separate samples of gas: ammonia, chlorine, and argon. Each sample hsa a volume of 10.00L, a temperature of 35.00 C. Rank these three gasses in order of increasing densitty and show how.

2. Consider trhee, separate samples of gas: helium, nitrogen, and neon. Each sample consists of 0.500 mol of the gas in a 10.00 L container at a temp of 5.00C. Rank tehse threee gasses in order of increasing average Kinetic energy.

3. N2(g) +3H2 ------> 2NH3 (g)

If 15.00L of nitrogen gas and 42.00L of hydrogen gas (both at 22.3 C and 50.00atm pressure) are allowed to react, what colume of ammonia gas (at 23.3 C and 50.00atm pressure) can be produced?

Answer 1

1. All the gases have same volume so they have same number of moles. So the with greater molar mass will have greater density. Among the given gases chlorine has highest molar mass and ammonia has least molar mass.

So the order of increasing density is

ammonia < argon < chlorine

2. average kinetic energy(3/2 kT) depends on tempearture only. All the three gases have same temperature so all they have same average kinetic energy.

3.