Question

The differential rate law for the reaction
H₂ (g) + I₂ (g) → 2HI (g) is
(a) - d[H₂]/dt = - d[I₂]/dt = - d[HI ]/dt
(b) d[H₂]/dt = d[I₂]/dt = 1/2 d[HI ]/dt
(c) 1/2 d[H₂]/dt = 1/2 d[I₂]/dt = - d[HI ]/dt
(d) -2 d[H₂]/dt = -2 d[I₂]/dt = d[HI ]/dt

Answer 1

(c ) is right answers

And thank and thank for the point

Answer 2

Let us answer it

Explanation:

Rate of reaction is actually :  time taken for reactants to form products"  .

The rate can also be defined as : increase in concentration of products with time

or

decrease in concentration of reactants with time .

For example : we have a reaction

A + B ----> AB

R = -d{AB }dt=d{A }/dt= d{B }/dt

If moles are present then :

aA + bB ---->x AB

Then the expression becomes :

R = -1/x d{AB }/dt=1/a d{A }/dt = -1/b d{B }/dt

Here negative sign indicates = decrease in concentration of reactants .

Here positive sign indicates : increase in concentration of products .

Now in the above asked question : option a is correct .