Question

# Nitric oxide reacts rapidly with unstable nitrogen trioxide NO3 to form NO2 NO(g) + NO3(g) →...

Nitric oxide reacts rapidly with unstable nitrogen trioxide NO3 to form NO2

NO(g) + NO3(g) → 2NO2(g)

Determine the rate law for the reaction and calculate the rate constant from the data below

 Experiment [NO]o (M) [NO3 ] (M) Initial reaction rate (M/s) 1 1.25x10-3 1.25x10-3 2.45 x 104 2 2.50x10-3 1.25x10-3 4.90 x 104 3 2.50x10-3 2.50x10-3 9.80 x 104

Going from experiment 1 to 2, [NO] gets doubled, [NO3] remains same and rate constant also gets doubled. Hence reaction is first order with respect to [NO].

Going from experiment 2 to 3, [NO3] gets doubled, [NO] remains same and rate constant also gets doubled. Hence reaction is first order with respect to [NO3].

Therefore, rate law is given by:

Rate = k[NO][NO3]

Consider experiment 1:

Rate = k[NO][NO3]

2.45 * 104 = k(1.25 * 10-3)(1.25 * 10-3)

k = 1.568 * 10-2 M-1s-1

#### Earn Coins

Coins can be redeemed for fabulous gifts.