(a)
Interpretation: Bond-line structures for reaction 1 and 2 should be formulated.
Concept introduction: Bimolecular substitution or
(b)
Interpretation: The nature of carbon at reactive site of the starting haloalkane should be identified.
Concept introduction:The carbon linked to one alkyl/carbon while other two
The carbon linked to two alkyl /carbons and one
The carbon linked to three alkyl groups/carbons and no
(c)
Interpretation:The manner in that different species would react and possible pathway that describes difference in rate between the reactions should be determined.
Concept introduction: Bimolecular substitution or
(d)
Interpretation: Hashed-wedged line structures to make a three-dimensional pathway to describe the trajectory should be drawn.
Concept introduction: Bimolecular substitution or
A general
Polar-aprotic solvents accelerate the rate of
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Organic Chemistry: Structure and Function
- The reaction of the alkene, ethylene, with H2 produces ethane as a product. However, the reaction is incredibly slow in the absence of a catalyst, such as platinum metal. What is the role of the catalyst in speeding up the reaction? Raising the activation energy by breaking the bonds of hydrogen molecules. By bringing together the hydrogen atoms and alkene on the same metal surface, thereby lowering the activation energy. By decreasing the number of reactive inermediates. By increasing the equilibrium constant for the reaction.arrow_forwardThe data below show the concentration of N2O5 versus time for the following reaction: N2O5 (g) → NO3 (g) + NO2(g) Time (s) [N2O5] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210arrow_forwardThe following is a nucleophilic substitution reaction of R-3-bromohexane with "SH. The experimental rate law for this reaction is Rate = k [R-3-bromohexane] [SH] H. H.C C. CH3 SH H2 Br H. The mechanism for this reaction is SN2 Draw the organic molecule(s) which is(are) formed in this reaction. Do not include molecules like H,O or HCl. Draw the specific configuration (R or S) at any chiral carbons within your product(s). If both configurations are formed in the product(s), draw both as separate molecules/products.arrow_forward
- Consider the following elimination reaction: Use the following data to identify the rate-determining step of the above reaction. Justify your rate law and overall reaction order based on this mechanistic step Experiment [Alcohol] [H+] Rate (M/s) 1 1.00 1.00 1.6 x 10-6 2 2.00 1.00 3.2 x 10-6 3 1.00 2.00 1.6 x 10-6 Knowing the overall reaction order, calculate the rate constant and the half-life of this reaction.arrow_forwardChemistry 1-bromo-1-methylcyclopropane + H2O → 1-methyl cyclopropane + HBr bromocyclopropane + H2O → cyclopropane + HBr Can I get a detailed description of the mechanism of these two reactions? (Specify each specific step and talk about how it happened.).arrow_forwardConsider this reaction: Br CH;OH Br-Br H3CO The mechanism proceeds through a first cationic intermediate, intermediate 1. Nucleophilic attack leads to intermediate 2, which goes on to form the final product. In cases that involve a negatively charged nucleophile, the attack of the nucleophile leads directly to the product. Br + CH3OH Br Intermediate 1 Intermediate 2 (product) In a similar fashion, draw intermediate 1 and intermediate 2 (final product) for the following reaction. OH + Br2 + HBr Br racemic mixturearrow_forward
- Consider this reaction: Br CH3OH Br-Br H3CO The mechanism proceeds through a first cationic intermediate, intermediate 1. Nucleophilic attack leads to intermediate 2, which goes on to form the final product. In cases that involve a negatively charged nucleophile, the attack of the nucleophile leads directly to the product. H. Br + CH;OH Br Intermediate 2 (product) Intermediate 1 In a similar fashion, draw intermediate 1 and intermediate 2 (final product) for the following reaction. OH + Br2 + HBr Br racemic mixturearrow_forwardThe activation energy for the gas phase decomposition of cyclobutane is 262 kJ. (CH₂) 4- →2 C₂H4 The rate constant at 721 K is 0.000401 /s. The rate constant will be 0.00338/s at K.arrow_forward16. Step 1 Step 2 Step 3 Students in a SCH4U class were examining the reaction between 2-bromo-2-methlypropane and water: (CH3)3CBr (aq) + H₂O (1)→ (CH3)3COH (aq) +H* (aq) + Br (aq) Their rate experiments show that the reaction is first order in (CH3)3CBr, but zero order in water. One of the students, Yuek-Fen, presented the following rate mechanism to her class for the above reaction. Determine if the mechanism below is plausible. Explain how you arrived at your decision. (CH3)3CBr (aq) → (CH3)3C (aq) + Br(aq) (CH3)3CH (aq) + H₂O (1)→ (CH3)3COH₂¹ (29) (fast) (CH3)3COH₂+ (aq) → 2H+ (aq) + (CH3)3COH (aq) Is this mechanism plausible? Explanation: (yes or no) (slow) (fast)arrow_forward
- 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 x2/2arrow_forward5. For the chlorination of ethane, represented by the equation: CH3CH3 + Cl2 + hv→ CH3CH2CI + HCI, the following radical-mediated mechanism has been proposed: Cl2 2 Cl· + CI - CH4 + Cl. → CH3· + HCI CH3: + Cl2 → CH3CI + Cl· k1, k.1 k2 k3 CH3* + Cl· 2CH3CI ka, k.4 Additionally, it has been possible to establish, under certain experimental conditions, that the reaction is first order with respect to the methane, and three halves with respect to chlorine. a) Classify the different steps of this mechanism (i.e. initiation, propagation, etc.). b) Derive the rate law for the chlorination of ethane, based on the mechanism proposed. c) Identify which is the rate-determining step. Justify your selection. d) Indicate which are the assumptions and approximations you used so that this model could work (i.e. pre- equilibrium condition, steady state approximation, neglecting the contribution of a step, etc.).arrow_forwardWhat is the overall reaction order of this reaction F2 + 2ClO2 → 2FClO2? Use the given reaction rate below.arrow_forward
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