An unknown liquid is composed of 34.31% C, 5.28% H, and 60.41% I. The molecular weight found by mass spectrometry is 210.06. What is the molecular formula of the compound?

검증된 단계별 안내

Calculate the moles of each element in 100 grams of the compound: For carbon (C), use the formula: moles of C = (34.31 g) / (12.01 g/mol). For hydrogen (H), use: moles of H = (5.28 g) / (1.008 g/mol). For iodine (I), use: moles of I = (60.41 g) / (126.90 g/mol).

Determine the mole ratio of the elements by dividing each element's moles by the smallest number of moles calculated in the previous step.

Round the mole ratios to the nearest whole number to find the empirical formula. If necessary, multiply all ratios by the same factor to get whole numbers.

Calculate the empirical formula mass by adding the atomic masses of the elements in the empirical formula.

Determine the molecular formula by dividing the given molecular weight (210.06 g/mol) by the empirical formula mass. Multiply the subscripts in the empirical formula by this factor to get the molecular formula.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the elements in a compound. To determine it, the percentage composition of each element is converted to moles, and then the ratios are simplified. This formula provides a foundational understanding of the compound's composition before deriving the molecular formula.

Molecular Weight

Molecular weight, or molar mass, is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic weights of all atoms in the molecular formula. In this question, the molecular weight obtained from mass spectrometry (210.06 g/mol) is crucial for determining the molecular formula from the empirical formula.

Molecular Formula

The molecular formula indicates the actual number of atoms of each element in a molecule of a compound. It can be derived from the empirical formula by multiplying the subscripts by a whole number, which is determined by dividing the molecular weight by the empirical formula weight. This formula provides a complete picture of the compound's composition.