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1.	In the following decomposition reaction,  2 N2O5 → 4 NO2 + O2 oxygen gas is produced at the average rate of 9.1 × 10-4 mol · L-1 · s-1. Over the same period, what is the average rate of the following: the production of nitrogen dioxide the loss of nitrogen pentoxide
	Solution: From the equation we see that for every 1 mole of oxygen formed, four moles of nitrogen dioxide are produced. Thus, the rate of production of nitrogen dioxide is four times that of oxygen: rate NO2 production = 4 × (9.1 × 10-4 mol · L-1· s-1)   = 3.6 × 10-3 mol · L-1· s-1 Nitrogen pentoxide is consumed at twice the rate that oxygen is produced: rate loss of N2O5 = 2× (9.1 × 10-4 mol · L-1· s-1)   = 1.8 × 10-3 mol · L-1· s-1
2.	Consider the following reaction: N2(g) + 3 H2(g) → 2 NH3(g) If the rate of loss of hydrogen gas is 0.03 mol · L-1· s-1, what is the rate of production of ammonia?
	Solution: From the balanced equation we see that there are 2 moles NH3 produced for every 3 moles H2 used. Thus: rate NH3 production = 2 3 × (0.03 mol · L-1· s-1)   = 0.02 mol · L-1· s-1