Question

Cl 2 and N 2 react according to the following equation

3Cl 2(g) + N 2(g) → 2NCl 3(g)
If 4 L of a stoichiometric mixture of chlorine and nitrogen are converted to nitrogen
trichloride under conditions of constant temperature and pressure what is the
volume of NCl 3(g) produced?

Answer 1

According to the balanced chemical equation, 3 moles of Cl2 react with 1 mole of N2 to produce 2 moles of NCl3. Therefore, the number of moles of NCl3 produced is (2/3) x n, where n is the number of moles of Cl2 in the original mixture.

Since the mixture is stoichiometric, the number of moles of Cl2 is equal to the number of moles of N2. Thus, the total number of moles of gas in the mixture is 2n.

Using the ideal gas law, we can relate the number of moles of gas to the volume of gas at constant temperature and pressure:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Since the temperature and pressure are constant, we can write:

V = (n/RT) x P

Substituting the expression for n above, we get:

V = [(2/3) x n / RT] x P

Therefore, the volume of NCl3 produced is [(2/3) x n / RT] x P.