Consider the below reaction mechanism:
Step 1: S(s) + O2(g) ⇌ SO2(g) fast; k1 = rate constant for forward reaction; k-1 = rate constant for reverse reaction
Step 2: SO2(g) + 1/2 O2(g) SO3(g) slow; k2 = rate constant
Step 3: SO3(g) + H2O(l) H2SO4(l) fast, k3 = rate constant
c) What is the rate law of the overall reaction?
I just don't understand how to rewrite the law without the intermediaries!