This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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3.1 Bond energy is the amount of energy required to break one mole of a specific type of bond in the gaseous state. 3.2 The C-Cl bond has a higher bond energy (340 kJ/mol) than the C-Br bond (280 kJ/mol). This difference is primarily due to the atomic size of chlorine versus bromine. Chlorine is a smaller atom than bromine, leading to a shorter and stronger C-Cl bond compared to the C-Br bond. Shorter bonds generally require more energy to break. 3.3 Step 1: Calculate the molar mass of chloromethane (CH_3Cl). M(CH_3Cl) = (1 × 12.011) + (3 × 1.008) + (1 × 35.453) M(CH_3Cl) = 12.011 + 3.024 + 35.453 = 50.488 g/mol Step 2: Calculate the number of moles of chloromethane in the sample. n = (m)/(M) = 5.05 g50.488 g/mol = 0.10002376 mol Step 3: Calculate the total energy required to break all bonds in 1 mole of chloromethane. Energy per mole = Total energy in sampleNumber of moles in sample = 157 kJ0.10002376 mol = 1569.62 kJ/mol Step 4: Set up an equation for the total bond energy in 1 mole of CH_3Cl. A molecule of CH_3Cl contains three C-H bonds and one C-Cl bond. Total energy per mole = (3 × E_C-H) + (1 × E_C-Cl) We know E_C-Cl = 340 kJ/mol from the table. 1569.62 kJ/mol = (3 × E_C-H) + 340 kJ/mol Step 5: Solve for the bond energy of the C-H bond (E_C-H). 3 × E_C-H = 1569.62 kJ/mol - 340 kJ/mol 3 × E_C-H = 1229.62 kJ/mol E_C-H = 1229.62 kJ/mol3 = 409.87 kJ/mol The bond energy of the C-H bond is 409.9 kJ·mol^-1. 3.4 Step 1: Identify the bonds present in 1 mole of bromomethane (CH_3Br) and their quantities. A molecule of CH_3Br contains three C-H bonds and one C-Br bond. Step 2: Use the calculated C-H bond energy from 3.3 and the given C-Br bond energy. E_C-H = 409.87 kJ/mol E_C-Br = 280 kJ/mol (from the table) Step 3: Calculate the total energy required to break all bonds in 1 mole of bromomethane. Total energy = (3 × E_C-H) + (1 × E_C-Br) Total energy = (3 × 409.87 kJ/mol) + (1 × 280 kJ/mol) Total energy = 1229.61 kJ/mol + 280 kJ/mol Total energy = 1509.61 kJ/mol The energy required to break all bonds in 1 mole of bromomethane is 1509.6 kJ·mol^-1. That's 2 down. 3 left today — send the next one.