Is first order in bro3⎻ , second order in br⎻, and zero order in h+. by what factor will the reaction rate change if the concentration of bro3⎻ is doubled, the concentration of br⎻ is halved, and the concentration of h+ is tripled ?

For a general reaction,

General expression for rate law  will be:

Here, r is rate of the reaction, k is rate constant, a is order with respect to reactant A and b is order with respect to reactant B.

The reaction is first order with respect to , second order with respect to and zero order with respect to .

According to above information, expression for rate law will be:

Or,

...... (1)

...... (2)

Dividing (2) by (1)

Or,

Thus, rate of the reaction also get doubled.

Or,

...... (3)

Dividing (3) by (1)

Or,

Thus, rate of reaction becomes 1/4th of the initial rate.

Since, the rate expression does not have concentration of , it is independent of it. Thus, any change in the concentration will not affect the rate of reaction and rate of reaction remains the same as in equation (1).

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

answer; i do believe the correct answer is (river); /// good luck