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QUESTION

# For the reaction: 4 NO2 (g) + O2 (g) 2 N2O5 (g) a) What is the rate of formation of N2O5 in terms of the rate of disappearance of O2? b) If the rate of disappearance of O2 = 0.0037 mol L-1s-1 what is the rate of disappearance of NO2?

4NO_2+O_2rarr2N_2O_5

(a)

Since 1 mole of O_2 is used up for every 2 moles of N_2O_5 formed the rate of formation of N_2O_5 will be twice the rate of disappearance of O_2.

(b)

Since 4 moles of NO_2 are used up for every mole of O_2 the rate of disappearance of NO_2 will be 4 times the rate of disappearance of O_2 = 4xx0.0037=0.0148 mol.l^(-1).s^(-1)