1. (3 points) For each of the following reactions, (1) balance the equations, (2) rewrite in terms of general reactants A and B and general products C, D, and E (if needed), and (3) write the rates of disappearance and formation in terms of concentration for each species, assuming that each reaction follows an-elementary rate law. If the reaction is reversible, the rate law should be written in terms of the thermodynamic equilibrium constant Kc (no krev in the final answer). \text { a) } \mathrm{CaCO}_{3}(\mathrm{~s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{CaCl}_{2} \text { (aq) }+\mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O} \text { (1) } \text { b) } \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \leftrightarrow \mathrm{SO}_{3}(\mathrm{~g}) \text { c) } \mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) \rightarrow \mathrm{Fe}(\mathrm{OH})_{2}(\mathrm{~s}) \text { d) } \mathrm{CuSO}_{4} \cdot 5 \mathrm{H}_{2} \mathrm{O}(\mathrm{s}) \leftrightarrow \mathrm{CuSO}_{4}(\mathrm{~s})+\mathrm{H}_{2} \mathrm{O} \text { (1) } \text { e) } \mathrm{Al}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{l}) \rightarrow \mathrm{AlBr}_{3}(\mathrm{~s})

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