A 10.0 L sealed reaction vessel at 450 K is charged with 2.00 mol of nitrogen gas and…
CHEMISTRY · Multi-part · A Level · Chemistry · Amount of substance · Amount of substance
Problem
A 10.0 L sealed reaction vessel at 450 K is charged with 2.00 mol of nitrogen gas and 6.00 mol of hydrogen gas. The gases react to form ammonia: N₂(g) + 3 H₂(g) → 2 NH₃(g). At 450 K, 30.0 % of the initial amount of nitrogen is converted to ammonia. Assume the temperature and volume remain constant and that all species behave ideally.
(1) Calculate the number of moles of each gaseous species present at equilibrium.
(2) Determine the total pressure inside the vessel at equilibrium.
(3) Calculate the partial pressure of ammonia at equilibrium.
(4) Using your results, determine whether the mole fraction of hydrogen gas has decreased by more than half of its initial value. Justify your answer with appropriate numerical evidence.