The hypochlorite ion oxidizes the iodide ion in aqueous solution as represented by the following equation: OCl–(aq) + I–(aq) → OI–(aq) + Cl–(aq) The rate law for this reaction is Rate = k [I-][OCl-]/[OH-]. The overall reaction order and the order with respect to OH- are?

At a certain temperature the rate of this reaction is second order in NH4OH with a rate constant of 0.0412M I 'S: NH4OH(aq) → NH3 (aq) + H2O (aq) Suppose a vessel contains NH4OH at a concentration of 1.36M. Calculate how long it takes for the concentration of NH4OH to decrease to 21.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ☐ Х

The reaction SO,Cl, (g) --> SO2 (g) + Cl2 (g) is first order. At 660 K it has a rate constant of 4.5 X 102s1. Determine the concentration of SO,Cl2 at 18.9 seconds, if the initial concentration is 0.562 M.

Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0015 M's : 2 NH, (g) - N, (g)+3 H, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of ammonia. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10

Consider a reaction: A + B C and the rate law expression: Rate = k [A]"[B]" If the reaction is zero order with respect to A and first order with respect to B, what are the values of m andn respectively. O m= 1 O m= 0 n = 1 O We need to know the concentrations of A and B to be able to answer this O We need to know the value of k to be able to answer this

Determine the rate law for the following reaction using the data provided. 2 NO(g) + O2(g) → 2 NO2(g) [NO]i (M) [02]i (M) Initial Rate (M-1s-1) 0.030 0.0055 8.55 x 10-3 0.030 0.0110 1.71 x 10-2 0.090 0.0055 2.56 x 10-2

Consider this reaction: 2Cl,0, (g) → 2C1, (g)+50, (g) At a certain temperature it obeys this rate law. rate = (0.221 5")[CL,0;] Suppose a vessel contains Cl,0, at a concentration of 1.11 M. Calculate how long it takes for the concentration of Cl,0, to decrease to 0.178 M. You may assume no other reaction is important. Round your answer to 2 significant digits.

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0084 M's : 2 HI (g) → H, (g) + I, (g) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. How much is left 1.0 s later? You may assume no other reaction is important. olo Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 18 Ar x10

The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 x 10¬4 mol/L-s. Au 2 HI(g) → H2 (g) + I2 (9) A[HI] Rate :k = 1.20 × 10¬4 mol/L ·s At a. If the initial HI concentration was 0.300 mol/L, calculate the concentration of HI at 24 minutes after the start of the reaction. Concentration = M b. How long will it take for all of the 0.300 M HI to decompose? Time = min

The reaction A+ B ---> C has the following rate law: Rate = k[A] [B]. If the concentration of A  is increased by a factor of 4 while the concentration of B is increased by a factor of 2, the rate will       increase by a factor of 8. increase by a factor of 16. decrease by a factor of 32. increase by a factor of 32.