Question

3.The rate constant for the reaction
2N2O5(g) = 2N2O4(g) + O2(g)
Is 4.98 x 10 -4 s-1. The order of reaction is

a.2
b.1
c.0
d.3​

Answer 1

Answer:

The order of reaction is 1

Explanation:

Since the unit of rate constant is $r^{-}$.The reaction is first order.

Answer 2

Given:

Rate constant for a reaction 2N2O5(g) = 2N2O4(g) + O2(g) is $4.98 * 10^{-4}$/s.

To Find:

The order of the given reaction.

Solution:

1. It is given that the order of the reaction is$4.98 * 10^{-4}$/s.

2. The units of the given rate constant are 1/s.

3. The formula of the rate constant is given by the expression,

Rate constant (k) = $(\frac{mol}{lit})^{1-n}s^{-1}$. where,

• The rate constant is denoted by k.
• n is the order of an equation.

4. Given rate constant has units of 1/s,

=> $(\frac{mol}{lit})^{1-n}$ = 0 (As only 1/s is present in the given constant).

=> n=1 ( Since$x^{0}$ = 1, For all values of x except 0).

5. As the value of n is 1, The order of the reaction will be 1.

• A first-order reaction is independent of the concentration of the solution.
• A First-order reaction is only dependent on the concentration/mass of the compound.

Therefore, the order of the reaction is 1 (OPTION B).