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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!