Organic Reactions

Step 1: Calculate the moles of benzaldehyde.
The molecular weight of benzaldehyde (MW = 106 g/mol) is given, so the moles of benzaldehyde is: Step 2: Calculate the theoretical yield.
Assuming a 1:1 molar ratio of benzaldehyde to product, the theoretical yield is: Step 3: Calculate the actual yield.
The actual yield is 5.2 g, so the percent yield is: Thus, the yield of the reaction is 98%.

Step 1: Understanding aromaticity.
Aromatic species are cyclic, planar molecules with conjugated double bonds that follow Huckel’s rule: having 4n + 2 π-electrons, where n is a non-negative integer.
Step 2: Analyzing the options.
- (A) The reaction of Cl with SbCl likely forms an aromatic species through an electrophilic aromatic substitution, where a chloride ion displaces another group to form a stable, aromatic intermediate.
- (B) The reaction of Br with AgBF involves a halide exchange, which is not likely to result in an aromatic species unless the resulting compound is conjugated. This reaction does not form an aromatic species.
- (C) The reaction of phenyl ketone (Ph-C(=O)Ph) with NaH (sodium hydride) could result in the formation of an aromatic species, as NaH can act as a base, removing a proton to form an aromatic species through a subsequent reaction.
- (D) The reaction of Na with an aromatic species generally results in a metal insertion, not the formation of an aromatic compound.
Step 3: Conclusion.
The correct reactions that result in aromatic species are (A) and (C).

Step 1: Analyze the reaction.
Trifluoroacetic anhydride (TFAA) is a powerful reagent used in esterification reactions, where it typically reacts with alcohols to form esters. The compound is reacted with hydrogen peroxide (H O ), which can oxidize the alcohol group in the presence of TFAA. The reaction results in the formation of an ester.
Step 2: Understanding the product formation.
In this case, the reaction results in the formation of an ester group (-O) replacing the -OH group. The methyl groups (Me) remain unchanged. The major product is the one shown in option (B), where the product contains an ester functionality.
Step 3: Conclusion.
Thus, the correct major product is (B).

Step 1: Understanding the reaction.
This reaction involves oxidation of glucose in the presence of bromine water (Br / H O) followed by treatment with hydrogen peroxide and ferric sulfate. The first step oxidizes the aldehyde group to a carboxylic acid, and the second step converts the cyclic structure into an open-chain form. The product formed from (D)-Glucose in these conditions is gluconic acid.
Step 2: Analyzing the compounds.
Among the compounds listed, only compound (B) is the one that, under identical conditions, will undergo the same oxidation and conversion process to form gluconic acid. The other structures differ in terms of hydroxyl and aldehyde positions.
Step 3: Conclusion.
Thus, the correct answer is (B).

Step 1: Understanding the reaction.
The given reaction involves an amine (a compound containing nitrogen) with an alcohol group, which is being protonated in the presence of an acidic condition (H ). Under acidic conditions, amines can undergo protonation, leading to the formation of an amine salt. The alcohol group may undergo dehydration or condensation reactions in the presence of acid, depending on the structure.
Step 2: Analyzing the product formation.
The major product in this case is formed due to protonation and the subsequent rearrangement or elimination, leading to a structure with a carbonyl group (C=O). This corresponds to an amide formation. Thus, the major product is likely to have an oxygen atom, representing the carbonyl group.
Step 3: Conclusion.
The correct major product is option (B) with the oxygen atom, corresponding to the amide formation.

Step 1: Understand the relationship for half-life.
The half-life of a reaction depends on its order. For a reaction of order , the half-life is given by: - For a zero-order reaction: - For a first-order reaction: - For a second-order reaction: Step 2: Apply the data.
We have two different initial concentrations (0.1 and 0.4 mol L ) and corresponding half-lives (200 and 50 s). If the reaction is first-order, the half-life should be independent of the initial concentration. This matches the observed data, suggesting the reaction is first-order.
Step 3: Conclusion.
The order of the reaction is 1, corresponding to option (B).

Step 1: Analyze the reaction.
The rate law for a reaction A + B Products is typically in the form:
Rate = k [A]^m [B]^n, where is the rate constant, and and are the reaction orders with respect to reactants A and B. The unit of the rate constant depends on the order of the reaction.
Step 2: Applying the units.
For a reaction with the overall order of 2, the unit of will be mol L s . This corresponds to option (C).
Step 3: Conclusion.
Thus, the overall order of the reaction is 2. The correct answer is (C) 2.

Step 1: Understanding oxidative addition.
The reactivity of a complex towards oxidative addition is influenced by the metal's oxidation state and the ligands attached. Complexes with low oxidation states and ligands that can easily accommodate changes in coordination geometry are more reactive.
Step 2: Analyzing the pairs.
Pair (II) and (IV) contain complexes with metal centers that are more likely to undergo oxidative addition due to their electronic configuration and the nature of the ligands.
Step 3: Conclusion.
Thus, the correct answer is (D) (II) and (IV).