How many moles of are in the system? — States of Matter and Gaseous State Chemistry Question

💡 Solution & Explanation

After opening all bulbs, the final pressure of $N_2$(g) is 33.5 mm Hg = 0.044 atm. Moles of $N_2$(g) = P_final × [V_A/T_A + V_B/T_B + V_C/T_C] / R = 0.044 × [1.642/300 + 1.642/200 + 1.642/80] / 0.0821 = 0.0125 mol. Since total initial moles of gas = 0.05 mol, and n_H2O = 0.015 mol, we have: n_CO2 = 0.05 - 0.015 - 0.0125 = 0.0225 mol.