Week 6 Discussion questionsAssume that two compounds, A and B, can react in one of two possible ways:A+BC+DA+BE+F

In a scenario where two compounds, A and B, can react in two different ways to form two different…

Answered: Week 6 Discussion questions Assume that…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 84GQ

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Hello i found the answer for part a to this question but i quickly need help with part b please. One pathway for the destruction of ozone in the upper atmosphere is O3(g) + NO(g) NO2(g) + O2(g) Slow NO2(g) + O(g) ---> NO(g) + O2(g) Fast Overall reaction: O3(g) + O(g) --> 2O2(g) Ea is 14.0 kJ/mol, for the uncatalyzed reaction: O3(g) + O(g) ---> 2O2(g) 1a) Ea for the same reaction, when catalyzed as above, is 11.9 kJ/mol.At -37°C, what is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction?(Assume the frequency factor A is the same for each reaction.) The ANSWER for this question is 2.91 1b) One of the concerns about the use of freons is that they will migrate to the upper atmosphere, where chlorine atoms can be generated by the reaction CCl2F2 --> CF2Cl + Cl (photolysis of Freon-12) Chlorine atoms can also act as a catalyst for the destruction of ozone.The activation energy for the reaction Cl + O3…
(a) Select all of the correct statements about reaction rates from the choices below. 1.The lower the rate of a reaction the longer it takes to reach completion.2 The rate of a reaction is independent of temperature.3 Slow reactions can be speeded up by raising the temperature.4. Reaction rates increase with increasing temperature.5. Solid catalysts do not affect reaction rates.6. Reactions involving very unstable combinations of chemicals have large rate constants.7. A balanced chemical reaction is necessary to relate
How do you determine the mechanism to these reactions to get the products?
Consider the following reaction and predict the new rate of the reaction if the concentration of A is doubled and the concentration of B was quadrupled. The new rate will be how many times greater than the original rate?
If the reaction rate of the following reaction is x, doubling the concentration of KCN would give what rate? KCN a no change in reaction rate b x2 x/2 2x e x2/2
The following reaction proceeds at a rate such that 4 mole of AA is consumed per minute. Given this, how many moles of CC are produced per minute? 2A+2B→4C
Which of the following is true given the information below? 3 H₂ (g) + N₂ (g) → 2NH₃ (g); ∆H = -22 kcal/mol A) The reaction is endothermic. B) The product is higher in energy than the reactants. C) Heat is released D) The activation energy for the reaction is negative.
Use the following data set for questions 3 and 4: A(aq) + B(aq) → Products Rxn # [A] [B] Rate of Loss of A 1 0.12 0.10 8.4 x 10-6 0.12 0.20 1.7 x 10-5 0.24 0.10 3.4 x 10-5 3. Determine the orders of reaction (m and n) for reactants A and B. Explain how you came to this conclusion or show your work. 4. Determine the rate constant (k) for the reaction above.
Use the information given in the following paragraph and energy diagram to answer questions 5-10. The mechanism for the reaction 2A D is illustrated in the following energy diagram where the X- axis is "reaction progress" and the Y-axis is "enthalpy". A is the reactant and D is the product. The reaction has a rate constant of 5.0x102² Mr¹ sec" when no catalyst is present. The equilibrium constant for the overall reaction at 25°C is K [D] = -=1.1×102. [A]² R D 9. You proposed the following mechanism for the overall reaction 2A D based on the energy diagram Step 1. A B (slow), with forward rate constant, k₂ (fast equilibrium), with forward rate constant, k₁, reverse rate constant k.] and equilibrium constant, K₁. Step 2. B 2C Step 3. A+2C D (fast), with forward rate constant, k3 Your classmate pointed out that your mechanism is incorrect. Why is your mechanism incorrect? a. Your mechanism does not incorporate the use of a catalyst b. Your mechanism is not consistent with the experimental…
Part A Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k[X]* [Y]3 %3D O The rate of reaction will increase by a factor of 6. O The rate of reaction will increase by a factor of 4. O the rate of reaction will increase by a factor of 8. O The rate of reaction will decrease by a factor of 4. O The rate of reaction will remain unchanged. Submit Request Answer
но HO HO HO 0 + ½ O, → + H,0 H H но OH ascorbic acid dehydroascorbic acid Vitamin C is oxidized slowly to dehydroascorbic acid by the oxygen in air. It is catalyzed by ions such as Cu*2 and Fe*3. The reaction can be followed by measuring the ultraviolet absorbance at 243 nm. Time (hours) Absorbance (A) 1/A In A - In A 0.75 1.3 -0.29 0.29 1 0.38 2.6 -0.97 0.97 2 0.19 5.3 - 1.7 1.7 3 0.095 11 - 2.4 2.4 29. What is the hybridization of carbon 1 (far left) and carbon 2 (middle) in this hydrocarbon: CH3CH=CH2? (A) sp³, sp (B) sp?, sp? (C) sp³, sp? (D) sp, sp?
#29) Arrhenius Equation and Activation Energy For the reaction: 2 NOCI(g) ------ > 2 NO(g) Cl2(g), the rate constant values were determined at two temperatures. At 127°C, the rate constant was 6.9 x 10-4/s while at 77°C, the rate constant was 9.3 x 10-6/s. (Note: Use the Arrhenius Equation pertaining rate constants at different temperatures in your calculations for this application) (29a) In blank #1, type-in your answer for the activation energy of the reaction. The unit is Joules, but enter only the value in numerals with three significant figures and with scientific notation using "E" instead of "x10^". (for example, the speed of light is 3.00E+8). (29b) In blank#2, type-in your answer for the rate constant for the same reaction at 202 degrees Celcius. No need to include units in your answer. Just enter the value of the answer in numerals with three significant figures and using scientific notation. Please use "E" instead of "x10^"; for example, the speed of light in wait +

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Week 6 Discussion questions Assume that two compounds, A and B, can react in one of two possible ways: A+B C+D A+B E+F