Question

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)`

Answer 1

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`