When the following reactions come to equilibrium, does the equilibrium mixture contain mostly reactants or mostly products?
(a) \(\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) \quad K_{c}=1.5 \times 10^{-10}\)
(b) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g) \quad K_{p}=2.5 \times 10^{9}\)
Text Transcription:
N2(g) + O2(g) \rightleftharpoons 2 NO(g) K_c = 1.5 X 10-10
2 SO2(g) + O2(g) \rightleftharpoons 2 SO3(g) K_p = 2.5 X 109
Step 1 of 5) We need to remember what a neutralization reaction is and calculate the amount of a substance needed to effect a certain change in pH. Plan For (a), we need to think about how acid can react with calcium carbonate, a reaction that evidently does not happen with acid and granite. For (b), we need to think about what reaction between an acid and CaO is possible and do stoichiometric calculations. From the proposed change in pH, we can calculate the change in proton concentration needed and then figure out how much CaO is needed. Solve (a) The carbonate ion, which is the anion of a weak acid, is basic (Sections 16.2 and 16.7) and so reacts with H+1aq2. If the concentration of H+1aq2 is low, the major product is the bicarbonate ion, HCO3 -. If the concentration of H+1aq2 is high, H2CO3 forms and decomposes to CO2 and H2O. Using the lake volume, we can calculate the number of moles of H+1aq2 at both pH values:
