Under certain conditions the decomposition of ammonia on a metal surface gives the following data:

[NH3] (M) 1.0 × 10−3 2.0 × 10−3 3.0 × 10−3

Rate (mol/L/h1) 1.5 × 10−6 1.5 × 10−6 1.5 × 10−6

Determine the rate equation, the rate constant, and the overall order for this reaction.

Rate equation :

2NH3(g) > N2(g) + 3H2(g)

The order for this reaction is a Zero order reaction.

Rate constant: Rate constant is therefore equals to the rate, given as 1.5*10^-6mol/L/hr.

Explanation:

Rate of a reaction is the number of moles of reactants converted or products formed per unit time.

Rate= change in concentration of the reactants or products /time taken.

From the data given, it is revealed that the rate of the reaction is the same irrespective of the change in the concentration of the reactant (NH3)

So, the reaction is a Zero order reaction.

Order of a reaction is the sum of the powers of the concentration of the reactants which appear in the rate equation

And since the above reaction is a zero order reaction, it means the concentration of the reactant does not affect the reaction.

Rate = k[NH3]^0

Rate = k

Rate = k = 1.5*10^-6mol/l/hr.

Thanks.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890