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]