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Chapter 3: Problem 31

Toluene on bromination in presence of light yields

Short Answer

Expert verified
Answer: The major product formed in the bromination of toluene in the presence of light is para-bromotoluene. For the given mass of toluene (20 g), 0.2377 moles of toluene are consumed, and 0.2377 moles of bromotoluene are formed in the reaction.

Step by step solution

01

Write the balanced chemical equation for the bromination of toluene

The bromination of toluene in the presence of light follows a free radical mechanism, and the major product formed is para-bromotoluene. The balanced chemical equation for the reaction is: C_7H_8 + Br_2 → C_7H_7Br + HBr
02

Calculate the moles of toluene consumed

To calculate the moles of toluene consumed, we first need to determine the molar mass of toluene: Molar mass of toluene (C_7H_8) = (7 * 12.01) + (8 * 1.01) = 84.14 g/mol Now, we can use the provided mass of toluene (20 g) and its molar mass to calculate the moles of toluene consumed: Moles of toluene = mass of toluene / molar mass of toluene = 20 g / 84.14 g/mol = 0.2377 mol
03

Determine the moles of bromotoluene formed

According to the balanced chemical equation, one mole of toluene reacts with one mole of bromine to yield one mole of bromotoluene. Since the reaction has a one-to-one stoichiometry and bromine is in excess, the moles of bromotoluene formed will be equal to the moles of toluene consumed: Moles of bromotoluene formed = moles of toluene consumed = 0.2377 mol
04

Formulate the final answer

In the bromination of toluene in the presence of light, the major product formed is para-bromotoluene, and the balanced chemical equation is given by C_7H_8 + Br_2 → C_7H_7Br + HBr. For the given mass of toluene (20 g), 0.2377 moles of toluene are consumed, and 0.2377 moles of bromotoluene are formed since bromine is in excess and the reaction has a one-to-one stoichiometry.

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