Concept explainers
(a)
To determine: The reason for less knocking tendency of isooctane than n-heptane.
Interpretation: The reason for less knocking tendency of isooctane than n-heptane is to be stated.
Concept introduction: The
(b)
To determine: An equation that shows abstraction of a hydrogen atom from tert-butyl alcohol by alkyl free radical and explanation for working of tert-butyl alcohol as an antiknock additive for gasoline.
Interpretation: An equation that shows abstraction of a hydrogen atom from tert-butyl alcohol by alkyl free radical is to be written and explanation for working of tert-butyl alcohol as an antiknock additive for gasoline is to be stated.
Concept introduction: The chemical reaction which proceeds through the formation of radicals is known as chain reaction. It involves three steps, initiation, propagation and termination. Generally, the initiation step occurs in the presence of light. The quantum yield of chain reactions is very high.
(c)
To determine: The explanation for high octane value of toluene and an equation that shows toluene react with an alkyl free radical to give relatively stable radical.
Interpretation: The explanation for high octane value of toluene and an equation that shows toluene react with an alkyl free radical to give relatively stable radical is to be stated.
Concept introduction: The chemical reaction which proceeds through the formation of radicals is known as chain reaction. It involves three steps, initiation, propagation and termination. Generally, the initiation step occurs in the presence of light. The quantum yield of chain reactions is very high.
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Chapter 4 Solutions
Organic Chemistry (9th Edition)
- A reaction proceeds by the following mechanism: NO2Cl+Cl→NO2Cl2 NO2Cl2→NO2+Cl2 What is the overall reaction? a. NO2Cl+Cl→NO2+Cl2 b. NO2Cl+Cl+NO2Cl2→NO2+Cl2+NO2Cl2 c. NO2Cl+Cl+2NO2Cl2→NO2+Cl2 d. NO2Cl+Cl+NO2+Cl2→2NO2Cl2arrow_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_forwardCyclohexene can react with hydrogen halides, HX, to yield the various halocyclohexanes, C6H11X. Rank HF, HCl, HBr, and HI in order from slowest reaction rate to fastest. Explain. Hint: What is the rate-determining step?arrow_forward
- El E2 Example Reaction Equation Rate Law Energy Diagram Why El or E2? Explainarrow_forwardWhen the concentration of reactant molecules is increased, the rate of reaction increases. The best explanation is: As the reactant concentration increases, the rate constant increases. the activation energy increases. the frequency of molecular collisions increases. the order of reaction increases. the average kinetic energy of molecules increases.arrow_forwardWhen first step of reaction is reversible/ not rate determining then how you can calculate the rate of reaction?arrow_forward
- 1). The coefficients in a reaction equation are not necessarily equal to the reaction orders, whereas the coefficients of an elementary step always equal the reaction orders of its rate law. Give one example and explain. 2. A reaction can be thermodynamically favorable, but kinetically unfavorable. What does that mean? When is a reaction thermodynamically or kinetically favorable or unfavorable? Choose a suitable reaction and draw energy diagrams to explain these concepts.arrow_forwardMatch the following descriptions to the appropriate term. Rate of reaction Rate law Rate constant Always has units of amount per time (e.g., M/s or M/min). Can have difurent unts Such as Ms, sor M depending on the reaction order. A formula that relates reactant concentration to reaction rate.arrow_forwardThe 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_forward
- What are all the main reaction mechanisms in organic chemistry?arrow_forwardproducts energy reactants Then answer the following questions about the chemical reaction. release Does this reaction release or absorb absorb energy? neither How many transition states occur during this reaction? yes Could this be an elementary reaction? no If you said this reaction could not be elementary, then how many steps are in its mechanism? If you said this reaction could not be elementary, then enter the number of the step in its mechanism which is rate- determining. For example, if the first step is the rate- determining step, enter "1" here.arrow_forwardDraw the order of reaction graphs (reaction rate vs the concentration) for [NO] and [H2]. Explain the difference between the two graphsarrow_forward
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