The oxidation of SO2 to SO3 is accelerated by NO2. The reaction proceeds according to: NO2(g) + SO2(g) → NO(g) + SO3(g) 2 NO(g) + O2(g) → 2 NO2(g) (a) Show that, with appropriate coefficients, the two reactions can be summed to give the overall oxidation of SO2 by O2 to give SO3. (d) Is this an example of homogeneous catalysis or heterogeneous catalysis?

Verified step by step guidance

1. Step 1: Write down the two given reactions: 1) NO2(g) + SO2(g) → NO(g) + SO3(g) 2) 2 NO(g) + O2(g) → 2 NO2(g)
2. Step 2: Add the two reactions together. To do this, ensure that the number of moles of each species on the reactant side equals the number of moles on the product side for any intermediates. In this case, NO2 and NO are intermediates.
3. Step 3: Cancel out the intermediates. Notice that NO2 appears as a reactant in the first reaction and as a product in the second reaction. Similarly, NO appears as a product in the first reaction and as a reactant in the second reaction. Cancel these intermediates.
4. Step 4: Write the net equation after canceling the intermediates. You should be left with the overall reaction: SO2(g) + 1/2 O2(g) → SO3(g).
5. Step 5: Determine the type of catalysis. Since both the reactants and the catalyst (NO2) are in the same phase (gaseous), this is an example of homogeneous catalysis.