# Calculate reaction orders.

#### lismx7

Hi I am new here and really hoping someone can help me with this question I have please...…

(B) Through experimentation, you note that at high temperatures ethyl chloride produces HCl and ethylene by the following reaction:

CH3CH2Cl(g) → HCl(g) + C2H4(g)

Using the rate data for the reaction at 650°C presented in the following table, calculate the reaction order with respect to the concentration of ethyl chloride (CH3CH2Cl). You must show your workings within your submission, and explain your reasoning. Your explanation should be a maximum of 200 words.

#### lismx7

And also this question please if anyone would be so kind to help me out.

(A) After experimentation you have determined the following rate equations:

1. Rate = k[H2] [NO]2

2. Rate = k[H2]2 [O2]

3. Rate = k[H2] [NO]

Identify the order of reaction for each of these rate equations. You must show your workings within your submission, and explain your reasoning. Your explanation should be a maximum of 200 words.

#### chemistrystudy

Order of a chemical reaction:
The order of a reaction is the power to which the concentration of a component is raised in the rate equation and overall order is the sum of the power of the concentration.
Thus for the reaction A+2B →3C+D,
if the experimental rate equation found as,
k = CACB
Then the reaction is first order with respect to A and first order with respect to B and the overall order of the reaction is 2.
But if the experimental rate lows is,
rate = k CA CB²
then the reaction is first order with respect to A and second order with respect to B, the overall order of the reaction is 3.
From the unit of rate constant we can given the idea about the order of the reaction

Examples

In chemical Kinetics unit of the rate constant in nth order reaction
= (unit of concentration)1-n (unit of time)⁻¹
Given unit of the rate constant = mol lit⁻¹sec⁻¹
= (unit of concentration)(unit of time)⁻¹
Compare the above two equation
We have 1 -n = 1
or, n = 0
Thus the reaction is zero order kinetics.