The decomposition of hydrogen peroxide &nbsp2H2O2(aq)&nbsp→ 2H2

The decomposition of hydrogen peroxide:  2H2O2(aq) → 2H2O(l) + O2(g) is catalyzed by I−(aq). The following mechanism has been proposed to explain the experimental rate law:  (1) H2O2 + I− ⇌ H2O + IO− slow  (2) H2O2 + IO− → H2O + O2 + I− fast Write the rate law for the above chemical reaction derived from the proposed mechanism. Use the format k*x^(m)*y^(n)…, where x = [H2O2], y = [H2O], z = [O2], u = [I−], v = [IO−].  5Br-(aq) + BrO3-(aq) + 6H+(aq) ‘ src=’’> 3Br2(l) + 3H2O(l)The above reaction is expected to obey the mechanism: BrO3-(aq) + H+(aq) HBrO3(aq)  Fast equilibrium HBrO3(aq) + H+(aq) H2BrO3+(aq)  Fast equilibrium H2BrO3+(aq) + Br-(aq) ‘ src=’’> (Br-BrO2)(aq) + H2O(l)  Slow (Br-BrO2)(aq) + 4H+(aq) + 4Br-(aq) ‘ src=’’> products  Fast Choose, from the list below, correct expressions for the overall rate law which are completely consistent with the above mechanism. Correct Incorrect -d[Br-]/dt = k[Br-][BrO3-][H+]2 Correct Incorrect -d[Br-]/dt = k[Br-][BrO3-][H+] Correct Incorrect k[H+][Br-][BrO3-]2 = -d[BrO3-]/dt Correct Incorrect -d[BrO3-]/dt = k[Br-] Correct Incorrect k[BrO3-][Br-][H+]2 = -d[H+]/dt Correct Incorrect -d[H+]/dt = k[Br-][BrO3-]2[H+]