<p>Chem 162 Quiz 1t Name______</p><p>Show work on all problems for full credit</p><p>-5 -1 1) (5 points) For the reaction, HI (g)  H2 (g) + I2 (g), the rate of formation of I2 is 2.0 x 10 M•s a) Symbolically write expressions for the rate of reaction in terms of each reactant and product. b) Calculate the rate of disappearance of HI. c) Determine the rate of reaction.</p><p>3 d) Calculate the final concentration of HI when [HI]0 = 5.00 M decomposes over 2.50 x 10 s. Assume that the rate is constant during the time interval.</p><p>2) (8 points) The rate of reaction between hemoglobin (Hb) and carbon monoxide (CO) was studied at 20 °C. The following data were collected with all the concentration units in mol/L. (2.21 mol/L = 2.21 x 10-6 mol/L)</p><p>Trial [Hb]0, [CO]0, Initial Rate, mol/L • s mol/L mol/L 1 2.21 1.00 0.619 2 4.42 1.00 1.24 3 4.42 3.00 3.71 a) Determine the orders of each reactant, Hb and CO. This can be calculated or stated in words for full credit.</p><p> b) Write the complete rate law for this reaction. c) Calculate the value of the rate constant, using trial 2. Be sure to include the units.</p><p> d) Calculate the initial rate for an experiment with [Hb]0 = 3.50 mol/L and [CO]0 = 1.80 mol/L. Time (ms) [Z] (M) 0.00 10.00 3) (8 points) Answer the following questions using the data table shown to the right for the reaction, Z ------> products. 0.10 8.00 0.32 5.56 a) Determine the order (0, 1, or 2) of [Z] using the half-life method. 0.60 4.00 0.80 3.33 b) Solve for one value of k base on your choice of order. Be sure to include the units of k. 1.10 2.67 1.50 2.11 c) Calculate the rate of reaction at [Z] = 0.75 M? 3.00 1.18 9.00 0.43 d) How long (in ms) will it take for [Z] = 0.05 M? 18.00 0.22 31.00 0.13 e) What you did for part a involves inductive logic. You now must demonstrate deductive logic. Eliminate one other order using the constant k method. Three k calculations are required. .</p><p>4) (4 points) Circle all the true statements.</p><p> a) Increasing temperature increases the rate of reaction by increasing the number of collisions.</p><p> b) A reaction is known to be 2nd order in [A]. When [A] is tripled (3x) the rate increases 27-fold (27x).</p><p> c) A linear plot of –[X]/t for X Y has a slope = 0. The order of [X] is 1st.</p><p> d) The overall order of a reaction with rate = k[A]2[B]-1[C]3 is 4.</p><p> e) If the slow step of a reaction requires light to start, the reaction is 1st order in the reactant.</p><p> f) For a 1st order reaction after 3 half-lives have passed, 87.5% of the reactant has reacted.</p><p> th -1 g) The time is takes a 0 order reaction to go from [A]0 = 10.0 M to [A] = 5.0 M with k = 2.0 x 10 M/s is 3.5 s. h) The initial rate method and integrated method for rate law determination are tools for examining the effect of the orientation/complexity of the collisions involved in a chemical reaction.</p>