Onsider the reaction, no2(g) + co(g) → no(g) + co2(g), for which the rate law has been determined to be: rate = k[no2]2[co]. which of the following statements is/are true? i: the rate of change of no2 is twice the rate of change of co. ii: doubling the concentrations of no2 and co simultaneously will increase the rate of the reaction by a factor of four. a) only ib) only iic) i and iid) none

A) Only I

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

Given:

k= rate constant

Order with respect to =2

Order with respect to = 1

I. The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Thus the rate of change of is twice the rate of change of .

II.  Doubling the concentrations of   and simultaneously will increase the rate of the reaction by a factor of four

Thus the rate increases by a factor of 8 and not 4.

Thus the correct statement is only  the rate of change of is twice the rate of change of .

because of all the things that happen around the us, many people get into arguments which sadly could get physical, but we should actually make a change for that.

the answer would be a