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.
ScanSolve AI Answer
Hey Mallikarjun, good to see you again. Here are the solutions to your questions: Question 1: The pair of species having same percentage composition of carbon, hydrogen, and oxygen. To have the same percentage composition, the compounds must have the same empirical formula. Step 1: Determine the molecular formula and then the empirical formula for each compound in the options. Option (1): CH_3COOH and C_6H_12O_6 For CH_3COOH: Molecular formula is C_2H_4O_2. Empirical formula: Divide subscripts by 2, which gives CH_2O. For C_6H_12O_6: Molecular formula is C_6H_12O_6. Empirical formula: Divide subscripts by 6, which gives CH_2O. Both compounds have the same empirical formula (CH_2O). Option (2): CH_3COOH and C_2H_5OH For CH_3COOH: Empirical formula is CH_2O. For C_2H_5OH: Molecular formula is C_2H_6O. Empirical formula: Cannot be simplified, so C_2H_6O. The empirical formulas are different. Option (3): HCOOCH_3 and C_12H_22O_11 For HCOOCH_3: Molecular formula is C_2H_4O_2. Empirical formula: CH_2O. For C_12H_22O_11: Molecular formula is C_12H_22O_11. Empirical formula: Cannot be simplified, so C_12H_22O_11. The empirical formulas are different. Option (4): C_6H_12O_6 and C_12H_22O_11 For C_6H_12O_6: Empirical formula is CH_2O. For C_12H_22O_11: Empirical formula is C_12H_22O_11. The empirical formulas are different. Step 2: Identify the option where both compounds have the same empirical formula. Option (1) is the only pair where both compounds have the same empirical formula (CH_2O). Therefore, they will have the same percentage composition of carbon, hydrogen, and oxygen. The final answer is Option (1). --- Question 2: A compound prepared as a model of had 4.6% iron by mass if the compound is known to contain a single iron atom, which of these values would be closest to its molar mass? Step 1: Identify the given information. Percentage of iron (Fe) by mass = 4.6\% Number of iron atoms per molecule = 1 Atomic mass of iron (Fe) ≈ 55.845 g/mol (we can use 56 g/mol for approximation as it's a multiple choice question). Step 2: Use the formula for percentage by mass. The percentage by mass of an element in a compound is given by: Percentage by mass of element = mass of element in one mole of compoundmolar mass of compound × 100\% Since there is one iron atom per molecule, the mass of iron in one mole of the compound is the atomic mass of iron. Let M be the molar mass of the compound. 4.6\% = Atomic mass of FeM × 100\% Step 3: Substitute the values and solve for M. Using the atomic mass of Fe = 56 g/mol: 4.6 = 56 g/molM × 100 M = 56 g/mol4.6 × 100 M = (5600)/(4.6) g/mol M ≈ 1217.39 g/mol Step 4: Compare the calculated molar mass with the given options. The calculated molar mass is approximately 1217.39 g/mol. The options are: (1) 1000 g mol^-1 (2) 1217 g mol^-1 (3) 1400 g mol^-1 (4) 1600 g mol^-1 The closest value to 1217.39 g/mol is 1217 g mol^-1. The final answer is Option (2). Drop the next question! 📸