Chap 9 questions

Chap 9 questions - Consider the following reaction in...

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Consider the following reaction in aqueous solution, 5Br - (aq) + BrO 3 - (aq) + 6H + (aq) --> 3Br 2 (aq) + 3H 2 O(l) If the rate of appearance of Br 2 at a particular moment during the reaction is 0.025 M s -1 , what is the rate of disappearance (in M s -1 ) of Br - at that moment? Consider the following reaction at 25 o C, (CH 3 ) 3 COH(l) + HCl(aq) --> (CH 3 ) 3 CCl(l) + H 2 O(l) The experimentally determined rate law for this reaction indicates that the reaction is first-order in (CH 3 ) 3 COH and that the reaction is first-order overall. Which of the following would produce an increase in the rate of this reaction? a. increasing the concentration of (CH 3 ) 3 COH b. increasing the concentration of HCl c. decreasing the concentration of HCl d. decreasing the concentration of (CH 3 ) 3 CCl e. It is impossible to tell. A certain first-order reaction has a rate constant, k, equal to 2.1 x 10 -5 s -1 at 355 K. If the activation energy for this reaction is 135 kJ/mol, calculate the value of the rate constant (in s -1 ) at 550 K. Which of the following influences the rate of a chemical reaction performed in solution? a. temperature b. activation energy c. presence of a catalyst d. concentrations of reactants e. All of the above influence the rate. The two diagrams below represent snapshots of a very small portion of a first-order reaction in which A molecules are being converted to B molecules (A --> B): Which of the following diagrams represents a snapshot of a very small portion of this system at t = 3 min?
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Laughing gas, N 2 O, can be prepared (ha, ha!) from H 2 and NO: H 2 (g) + 2 NO(g) --> N 2 O(g) + H 2 O(g) A study of initial concentration (ha, ha!) versus initial rate at a certain temperature yields the following data for this reaction (ha, ha!): [H 2 ], M [NO], M initial rate, M s -1 0.1000 0.5000 2.560 x 10 -6 0.2000 0.3000 1.843 x 10 -6 0.1000 0.3000 9.216 x 10 -7 0.2000 0.6000 7.373 x 10 -6 Which of the following is the correct rate law for this reaction (ha, ha!)? a. Rate = k[H 2 ][NO] 2 b. Rate = k[H 2 ][NO] c. Rate = k[NO] 2 d. Rate = k[H 2 ] 2 e. Rate = k Iodine-131, a radioactive isotope of iodine, is used medicinally as a radiotracer for the diagnosis and treatment of illnesses associated with the thyroid gland. The half-life of iodine-131 is 7.0 x 10 5 seconds. If a patient is given 0.45 g of iodine-131, calculate how long it would take (in seconds) for 90.0% of the iodine-131 to decay. Recall: radioactive decay is a first-order process. Consider a reaction which is first-order in A and first-order in B , A + B --> Products Rate = k[ A ][ B ] What are the relative rates of this reaction in the vessels shown below. Note: each vessel has the same volume.
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a. III > I = IV > II b. I > III > II > IV c. IV > II > III > I d. II > IV > I > III e. III > I > IV > II The complex ion, [Cr(NH 3 ) 5 Cl] 2+ , reacts with OH - ion in aqueous solution, [Cr(NH 3 ) 5 Cl] 2+ (aq) + OH - (aq) --> [Cr(NH 3 ) 5 (OH)] 2+ (aq) + Cl - (aq)
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Chap 9 questions - Consider the following reaction in...

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