Organic Chemistry
5th Edition
ISBN: 9780078021558
Author: Janice Gorzynski Smith Dr.
Publisher: McGraw-Hill Education
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Chapter 6, Problem 6.20P
Draw an energy diagram for a two-step reaction,
compounds is
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For a reaction that follows the general rate law Rate = KIAJ [B), what will happen to the rate of reaction if the concentration of A and B are increased by a factor of 6?
O The rate will increase by a factor of 36.00.
O The rate will decrease by a factor of 1/6.00.
O The rate will decrease by a factor of 1/36.00.
O The rate will increase by a factor of 6.00.
4. What is the difference between catalysts and
intermediates?
Catalysts may appear in rate law expressions.
Intermediates may appear in rate law expres-
sions.
A catalyst gets made by an early step in a mech-
anism, but used up again in a later step.
An intermediate gets made by an early step in a
mechanism, but used up again in a later step.
Can someone please help with question 10a
Chapter 6 Solutions
Organic Chemistry
Ch. 6 - Problem 6.1 Classify each transformation as...Ch. 6 - Prob. 6.2PCh. 6 - Problem 6.3 By taking into account...Ch. 6 - Problem 6.4 Use curved arrows to show the movement...Ch. 6 - Problem 6.5 Follow the curved arrows and draw the...Ch. 6 - Prob. 6.6PCh. 6 - Problem 6.7 Use the values in Table 6.2 to...Ch. 6 - Prob. 6.8PCh. 6 - aWhich Keq corresponds to a negative value of G,...Ch. 6 - Given each of the following values, is the...
Ch. 6 - Given each of the following values, is the...Ch. 6 - The equilibrium constant for the conversion of the...Ch. 6 - Prob. 6.13PCh. 6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6 - Draw an energy diagram for a reaction in which the...Ch. 6 - Prob. 6.17PCh. 6 - Prob. 6.18PCh. 6 - Problem 6.19 Consider the following energy...Ch. 6 - Draw an energy diagram for a two-step reaction,...Ch. 6 - Which value if any corresponds to a faster...Ch. 6 - Prob. 6.22PCh. 6 - Problem 6.23 For each rate equation, what effect...Ch. 6 - Prob. 6.24PCh. 6 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 6.29PCh. 6 - 6.30 Draw the products of each reaction by...Ch. 6 - 6.31 (a) Add curved arrows for each step to show...Ch. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Calculate H for each reaction. a HO+CH4CH3+H2O b...Ch. 6 - Homolysis of the indicated CH bond in propene...Ch. 6 - Prob. 6.37PCh. 6 - Prob. 6.38PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 6.40PCh. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 6.45PCh. 6 - Draw an energy diagram for the Bronsted-Lowry...Ch. 6 - Prob. 6.47PCh. 6 - Indicate which factors affect the rate of a...Ch. 6 - Prob. 6.49PCh. 6 - 6.50 The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 6.51PCh. 6 - Prob. 6.52PCh. 6 - The conversion of (CH3)3Cl to (CH3)2C=CH2 can...Ch. 6 - 6.54 Explain why is more acidic than , even...Ch. 6 - Prob. 6.55PCh. 6 - Prob. 6.56PCh. 6 - Prob. 6.57PCh. 6 - Although Keq of equation 1 in problem 6.57 does...Ch. 6 - Prob. 6.59P
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- . Account for the increase in reaction rate brought about by a catalyst.arrow_forwardWhy awe elementary reactions involving three or more reactants very uncommon?arrow_forwardConsider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.arrow_forward
- Draw an energy diagram for a two-step reaction, A -> B -> C, where the relative energy of these compounds is C < A < B, and the conversion of B ? C is rate-determining.arrow_forwardDraw an energy diagram for a two-step reaction, A → B → C, where the relative energy of these compounds is C < A < B, and the conversion of B→ C is rate-determining.arrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?arrow_forward
- Consider the following reaction: (a) The rate law for this reaction is first order in NO₂(g) and first order in O3(g). What is the rate law for this reaction? O Rate = k [NO₂(g)] [03(9)] Rate = k [NO₂(g)]² [03(9)] O Rate = k [NO₂(g)] [03(9)]² O Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(9)] (b) If the rate constant for this reaction at a certain temperature is 73200, what is the reaction rate when [NO₂(g)] = 0.973 M and [O3(9)] = 1.42 M? Rate = 2 NO₂(g) + 03(g) → N₂05(9) + O₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.95 M while the concentration of O3(g) is 1.42 M? M/sarrow_forward4. The reaction 2NO(g) + Oz(g) - 2NO:(g) has the following rate law: Rate - kjO2]|NO]2. If the concentration of NO is reduced by a factor of two, the rate will A. double C. be reduced by one-half D. be reduced by one-quarter B. quadruple 5. The rate of a reaction is found to double when the concentration of one reactant is quadrupled. The order of the reaction with respect to this reactant is A. first C. third D. one-half B. secondarrow_forwardHere are representations of a reaction: A + B --> products Unshaded spheres represent A molecules. Shaded spheres represent B molecules. Trial 1 Trial 2 Trial 3 Trial 4 Rate = 1 Rate = 1 Rate = 4 Rate = 4arrow_forward
- Consider this reaction: NH₂OH(aq) → NH3(aq) + H₂O (aq) At a certain temperature it obeys this rate law. =(2.24 s¯¹) [NH₂OH] rate olo Suppose a vessel contains NH OH at a concentration of 1.38M. Calculate how long it takes for the concentration of NH4OH to decrease to 13.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. S 0 OHarrow_forwardConsider the following reaction: (a) The rate law for this reaction is first order in HBr(g) and first order in O₂(g). What is the rate law for this reaction? Rate = k [HBr(g)] [O₂(g)] O Rate = k [HBr(g)]² [O₂(g)] O Rate = k [HBr(g)] [O₂(g)]² O Rate = k [HBr(g)]² [0₂(g)]² O Rate = k [HBr(g)] [O₂(g)]³ O Rate = k [HBr(g)]4 [0₂(g)] (b) If the rate constant for this reaction at a certain temperature is 11500, what is the reaction rate when [HBr(g)] = 0.00379 M and [O₂(g)] = 0.00876 M? Rate = 4 HBr(g) + O₂(g) → 2 H₂O(g) + 2 Br₂(g) M/s. Rate = (c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00758 M while the concentration of O₂(g) is 0.00876 M? M/Sarrow_forwardDoes increasing the amount of a reactant (NOT THE CONCENTRATION) from say 2.5mL to 5.0mL of Na2S2O3 increase the rate of a reaction or lower it?arrow_forward
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