For the reaction: 2 H2 + 2 NO → N2 + 2 H2O the observed rate expression, under some conditions, is: rate = k[H2][NO]2 Which of the following mechanisms are consistent with these data? Select all that are True. step 1 H2 + 2 NO → N2O + H2O (slow) step 2 N2O + H2 → N2 + H2O (fast) step 1 2 H2 + 2 NO → N2 + H2O step 1 NO + NO ⇌ N2O2 (fast) step 2 N2O2 + H2 → N2 + H2O + O (slow) step 3 O + H2 → H2O (fast) step 1 H2 + NO ⇌ H2ON (fast) step 2 H2ON + NO → N2 + H2O2 (slow) step 3 H2O2→ H2O + O (fast) step 4 O + H2 → H2O (fast)

Step 1 H2 + 2 NO → N2O + H2O (slow)

step 2 N2O + H2 → N2 + H2O (fast)

Explanation:

It is known that the slowest step in a reaction is the rate determining step in a sequence of reactions (reaction mechanism).

We have two important pieces of information in the question to guide our decision making process.

The overall reaction equation, and the rate expression. The two;

2 H2 + 2 NO → N2 + 2 H2O and rate = k[H2][NO]2 all support the answer given above.

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml