The rate of disappearance of HCl was measured for the following reaction: CH3OH (aq) + HCl (aq) --> CH3Cl (aq) + H₂O (1) The following data (table on this page, graph on the next page) was collected. 1. Determine the order with respect to HCL. Briefly explain your reasoning. 2. Given the reaction is first order with respect to CH,OH, determine the rate law expression. 3. Using two data points, calculate the rate constant k. time (min) 0.0 54.0 107.0 215.0 430.0 [HC] (M) In (HCI) (M) 1/[HC] (M) 1.85 0.615185639 0.540540541 1.58 0.457424847 0.632911392 1.36 0.3074847 0.735294118 1.02 0.019802627 0.980392157 0.58 -0.544727175 1.724137931

During kinetic studies, the following reaction was determined to be first order in respect to CH3OH and second order in respect to HCl.  What is the overall order for the reaction?   CH3OH(aq) +  HCl(aq) ---->  CH3Cl(aq)  +  H2O(i)

At a certain temperature the rate of this reaction is second order in NH OH with a rate constant of 0.0123 M¹s¹: NH,OH (aq) → NH, (aq)+H,O(aq) Suppose a vessel contains NH OH at a concentration of 0.690 M. Calculate the concentration of NH OH in the vessel 790. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. X

The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)

A chemical engineer is studying the rate of this reaction. 2NH3 (g) → N₂ (g)+ 3H₂ (g) She fills a reaction vessel with NH3 and measures its concentration as the reaction proceeds. Here's a graph of her data: (W) [EHN] 0.20- 0.15- 0.10- 0.05- 0_ 20 60 t (s) 80 100

For the reaction CH, OH(aq) + H* (aq) + Cl¯ (aq) → CH₂ Cl(aq) + H₂O(1) the value of [H*] was measured over a period of time. Given the data in the table, find the average rate of disappearance of H* (aq) for the time interval between each measurement. Interval: 0 s to 30.0 s reaction rate: 6.5 X10-3 reaction rate: Incorrect Interval: 30.0 s to 60.0 s 4.8 x10-3 Incorrect t (s) 0 30.0 60.0 117.0 [H+] (M) 2.34 2.12 2.00 1.83 M/s M/S Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books

- 1 At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0968 s 2N,O; (g) → 2N,04 (g) + O2 (g) Suppose a vessel contains N,0g at a concentration of 1.07M. Calculate the concentration of N,O, in the vessel 6.40 seconds later. '2 You may assume no other reaction is important. Round your answer to 2 significant digits.

A scientist already determined the rate of the reaction is first order with respect to I - . Determine the rate law and the value of k for the following reaction using the data provided. Hint, you only need to find the reaction order for S2O82⁻  because it is first order for I - . After you find the reaction order for S2O82⁻  you need to calculate k.   S2O82⁻ (aq) + 3 I⁻ (aq)  →   2 SO42⁻ (g) + I3⁻ (aq) [S2O82⁻ ]i (M) [I⁻ ]i (M) Initial Rate (M -1 s -1 )  0.30 0.42 4.54  0.44 0.42 6.65     Rate = 120 M-2s-1 [S2O82⁻]2[I⁻]     Rate = 195 M-3s-1 [S2O82⁻]2[I⁻]     Rate = 86 M-2s-1 [S2O82⁻][I⁻]     Rate = 23 M-1/2s-1 [S2O82⁻][I⁻]     Rate = 36 M-1s-1 [S2O82⁻][I⁻]

Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś