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

Answer:

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#