Determining reaction order : Rate Laws(Chemistry)
The reaction of nitric oxide with hydrogen at 1280C is as follows:
2NO(g) +2H2 (g) -> N2(g) + 2H2O(g)
From the following experimental data, determine the rate law and the rate constant.
30 POINTS!

The order of the reaction is 4.

The rate law of the reaction will be :

Rate constant of the reaction: k =

Explanation:

Let the stoichiometric coefficient of the NO and in rate law be x and y .

Rate of the reaction is given  by :

1) When ,

R =  0.00600 M/s

..[1]

2) When ,

R =  0.144 M/s

..[2]

3) When ,

R =  0.0120 M/s

..[3]

Dividing [1] and [3]

y = 1

Dividing [1] and [2]

x = 3

The order of the reaction = x + y = 3 + 1 = 4

The rate law of the reaction will be :

Rate constant of the reaction: k

When ,

R =  0.00600 M/s

..[1]

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

they are made of gases.

they have a spherical shape.

they make energy through fusion.