Consider the reaction of A(g) + B(g) + C(g) => D(g) for whichthe following data were obtained:
Experiment Initial [A], mol/L Initial [B], mol/L Initial [C], mol/L Initial rate, mol/L. s
1 0.0500 0.0500 0.0100 6.25 x 10-3
2 0.100 0.0500 0.0100 2.50 x 10-2
3 0.100 0.100 0.0100 1.00 x 10-1
4 0.0500 0.0500 0.0200 1.25 x 10-2
What is the rate law for the reaction?
1. rate= k[A][B][C]
2. rate= k[A]2[B]2[C]
3. rate= k[A]2[B][C]
4. rate= k[A]2[B]2
5. rate= k[A][B]

rate= k[A]²[B]²[C]

Explanation:

When concentration of A is increased two times ,keeping other's concentration constant , rate of reaction becomes 4 times .

So rate is proportional to [A]²

When concentration of B is increased two times , keeping other's concentration constant,rate of reaction becomes 4 times.

So rate is proportional to [B]²

When concentration of C is increased two times , keeping other's concentration constant, rate of reaction becomes 2 times.

So rate is proportional to [C]

So rate= k[A]²[B]²[C]

if you mean hydrogen and oxygen then water is the product