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
To find the relative molecular mass of a compound with the empirical formula CH_2O, we first calculate the empirical formula mass (EFM). Step 1: Calculate the empirical formula mass (EFM) of CH_2O. Given atomic masses: Relative atomic mass of Hydrogen (H) = 1.0 Relative atomic mass of Carbon (C) = 12.0 Relative atomic mass of Oxygen (O) = 16.0 The empirical formula CH_2O contains 1 carbon atom, 2 hydrogen atoms, and 1 oxygen atom. EFM = (1 × C) + (2 × H) + (1 × O) EFM = (1 × 12.0) + (2 × 1.0) + (1 × 16.0) EFM = 12.0 + 2.0 + 16.0 EFM = 30.0 Step 2: Determine which of the given options is a multiple of the empirical formula mass. The relative molecular mass (RMM) of a compound is always a whole number multiple (n) of its empirical formula mass: RMM = n × EFM We need to find an option that, when divided by 30.0, gives a whole number. Let's check the options: (a) 42 ÷ 30.0 = 1.4 (not a whole number) (b) 45 ÷ 30.0 = 1.5 (not a whole number) (c) 126 ÷ 30.0 = 4.2 (not a whole number) (d) 180 ÷ 30.0 = 6 (a whole number) Only option (d) is a whole number multiple of the empirical formula mass. This means that for this compound, n=6, and its molecular formula would be (CH_2O)_6, which is C_6H_12O_6. The correct option is d). d) 180 That's 2 down. 3 left today — send the next one.