As \(\mathrm{NH}_{3}(g)\) is decomposed into nitrogen gas and hydrogen gas at constant pressure and temperature, the volume of the product gases collected is twice the volume of \(\mathrm{NH}_{3}\) reacted. Explain. As \(\mathrm{NH}_{3}(g)\) is decomposed into nitrogen gas and hydrogen gas at constant volume and temperature, the total pressure increases by some factor. Why the increase in pressure and by what factor does the total pressure increase when reactants are completely converted into products? How do the partial pressures of the product gases compare to each other and to the initial pressure of \(\mathrm{NH}_{3}?\)

In the decomposition of ammonia gas (\(NH_3\)) to nitrogen gas (\(N_2\)) and hydrogen gas (\(H_2\)), the volume of the product gases is twice the volume of the reacted ammonia gas under constant pressure and temperature. This is because the stoichiometry of the reaction dictates that one mole of \(NH_3\) produces 1/2 mole of \(N_2\) and 3/2 moles of \(H_2\), resulting in a volume ratio of 2. When the reaction occurs at constant volume and temperature, the total pressure increases by a factor of 2. This is due to the increase in the number of moles of gaseous products compared to the reactants. The partial pressure of \(N_2\) is half the initial pressure of \(NH_3\), and the partial pressure of \(H_2\) is three times the initial pressure of \(NH_3\).