A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? step 1: A + B → 2C + D (slow) step 2: C → E (fast) step 3: D → 2F (fast)

rate = l[A][B]

Explanation:

We are given the information that step 1:  A + B → 2C + D is the the rate determinng steps, while the other 2 are fast in the reaction mechanism.

The rate law which is what we need to determine in this question is dependent on the  the slowest step,  

Therefore, the rate law will be a second order overall and dependent on the concentrations of A and B:

rate = k [A][B]

i'm pretty sure it is letter c.) car

oxygen, selenium, tellurium, and polonium.

they're all from the same group as sulfur (group 16).