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Unformatted text preview: Key of Worksheet for Chemical Kinetics 1. For the reaction shown below, the rate is expressed as 1 6 [ H 2 O ] t . 6 CH 2 O + 4 NH 3 ( CH 2 ) 6 N 4 + 6 H 2 O An equivalent expression is: (e) a. 1 2 [( CH 2 ) 6 N 4 t b. 6 [ CH 2 O ] t c. - 6 [ CH 2 O ] t d. - 1 6 [ H 2 O ] t e. - 1 4 [ NH 3 ] t 2. For this reaction X 2 + Y + Z XY + XZ , the mechanism goes as follows: X 2 + Y XY + X (very slow) X + Z XZ (very fast) What is the rate law for this reaction? (d) a. rate = k [X 2 ][Y][Z] b. rate = k [X 2 ] c. rate = k [X 2 ][Z] d. rate = k [X 2 ][Y] 3. Complete the following statements relating to the production of ammonia by the Haber process, for which the overall reaction is: N 2 (g) + 3 H 2 (g) 2 NH 3 (g). a. The rate of disappearance of N 2 is times the rate of disappearance of H 2 . b. The rate of formation of NH 3 is times the rate of disappearance of H 2 . c. The rate of formation of NH 3 is times the rate of disappearance of N 2 . (a) one-third; (b) two-thirds; (c) two 4. What is/are the rate-determining step of the reaction mechanism listed below. The overall rate is dependent on the pH of the solution. ClO- (aq) + Br- BrO- (aq) + Cl- Step 1: ClO- (aq) + H 2 O HClO- (aq) + OH- (aq) Step 2: Br- (aq) + HClO- (aq) HOBr (aq) + Cl- (aq) Step 3: OH- (aq) + HOBr (aq) H 2 O + BrO- (aq) a. Step 1 b. Step 2 c. Step 3 d. More than one Suppose...
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This note was uploaded on 03/29/2010 for the course CHEMISTRY 230 taught by Professor Gottfried during the Fall '10 term at University of Michigan.
- Fall '10