With the reaction, determine the masses of HSO_3NH_2 required to produce 0.135 g of N_2(g) collected in a burette above water. How do you calculate the volume that this mass of N_2(g) would occupy at 23.4°C and 7.10*10^2 mmHg barometric pressure?

HSO_3NH_2(aq) + NaNO_2(aq) -> NaHSO_4(aq) + N_2(g) + H_2O(l)

1 Answer
Apr 9, 2017

Calculate the masses from the related molar amounts. Calculate the volume of N_2 from the ideal gas laws.

Explanation:

The balanced equation shows that every mole of N_2 requires one mole of HSO_3NH_2. 0.135g of N_2 is (0.135/28) = 0.00482 moles of N_2.

This requires (0.00482 * 97) = 0.468g of HSO_3NH_2 and (0.00482 * 53) = 0.42555g of NaNO_2.

The volume of N_2 produced is V = ((n*R*T)/P)

P = 710/760 = 0.934atm, R = 0.0821 L-atm/K-mol, T = 296.6’K, n = 0.00482 moles, V = Liters

V = ((0.00482*0.0821*296.6)/0.934) ; V = 0.126L