Answer:
(a).
[tex]order \: of \: A = 2 \\ order \: of \:B = 0 \\ rate = k[A] {}^{2} [B][/tex]
(b)
[tex]0.32 \times {10}^{ - 3} = k {(0.12)}^{2} (0.15) \\ k = 0.148 \: {mol}^{ - 2} {dm}^{6} {s}^{ - 1} [/tex]
(c). The rate increases because kinetic energy of reactant molecules increases.
