Consider the initial rates measured for reaction 2 NO + O 2 → 2 NO 2

Trial 1 2 3
[NO] (in M) 0.010 0.010 0 .030
[O2] (in M) 0.010 0.020 0 .020
Initial rate (M/s) 2.5 5.0 45 .0
Determine the value of x and y in the rate law for this reaction: r = k[NO] x[O 2] y
x = 0, y = 2
x = 2, y = 1
x = 1, y = 1
x = 2, y = 2
x = 1, y = 2

x = 2, y = 1

Explanation:

solving for x using trial 2 & 3:

using the basic rate law equation r = k [A]^x[B]^yset the initial rate = k[NO]^x[O2]^y and plug values inyou can cancel out the O2 because they have the same value -> you should be selecting the trials where only one independent value (in this case, NO or O2) changesthis is basically the same thing for y

solving for y using trial 1 & 2:

A. tetrahedral

B. angular or bent

C. angular

D. trigonal planar

E. linear

F. linear

Explanation: