Question

# 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} \text { (s) }+\mathrm{HCl} \text { (aq) } \rightarrow \mathrm{CaCl}_{2} \text { (aq) }+\mathrm{CO}_{2} \text { (g) }+\mathrm{H}_{2} \mathrm{O} \text { (l) } \text { b) } \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \leftrightarrow \mathrm{SO}_{3} \text { (g) } \text { c) } \mathrm{Fe}^{2+}(90)+\mathrm{OH}^{-}(\mathrm{ad}) \rightarrow \mathrm{Fe}(\mathrm{OH} \text { (s) } \text { d) } \mathrm{CuSO}_{4}-5 \mathrm{H}_{2} \mathrm{O} \text { (s) } \leftrightarrow \mathrm{CuSO}_{4} \text { (s) }+\mathrm{H}_{2} \mathrm{O} \text { (l) } \text { e) } \mathbf{A l}(\mathrm{s})+\mathbf{B r} 2(1) \rightarrow \mathbf{A l B r} \text { (s) }  Fig: 1  Fig: 2  Fig: 3  Fig: 4  Fig: 5  Fig: 6