The ratio of oxygen to carbon by mass in carbon monoxide is 1.33:1.00. Find the formula of an oxide of carbon in which the ratio by mass of oxygen to carbon is 2.00:1.00.

Verified step by step guidance

1. Determine the molar mass of carbon (C) and oxygen (O). Carbon has a molar mass of approximately 12.01 g/mol, and oxygen has a molar mass of approximately 16.00 g/mol.
2. Calculate the mass of oxygen in carbon monoxide (CO) using the given mass ratio in CO, which is 1.33:1.00. This means for every 1.00 g of carbon, there are 1.33 g of oxygen.
3. Using the molar masses, convert the masses in carbon monoxide to moles to confirm the 1:1 stoichiometry in CO: 1.33 g of oxygen divided by its molar mass gives the moles of oxygen, and 1.00 g of carbon divided by its molar mass gives the moles of carbon.
4. Apply the new mass ratio of oxygen to carbon, which is 2.00:1.00, to find the formula of the new oxide. For every 1.00 g of carbon, there are now 2.00 g of oxygen.
5. Convert these masses into moles using their respective molar masses, and find the simplest whole number ratio of moles of oxygen to moles of carbon to determine the empirical formula of the new carbon oxide.

Key Concepts

Molar Mass

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 masses of all atoms in a chemical formula. Understanding molar mass is essential for converting between mass and moles, which is crucial for determining the ratios of elements in compounds.

Mass Ratio

The mass ratio of elements in a compound is the ratio of the mass of one element to the mass of another element. In this context, it helps to compare the relative amounts of carbon and oxygen in carbon monoxide and the desired oxide. This concept is fundamental for deriving the empirical formula based on the given mass ratios.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of atoms of each element in a compound. It is derived from the mass ratios of the elements and is crucial for identifying the composition of a compound. In this question, finding the empirical formula of the oxide of carbon requires applying the mass ratio of oxygen to carbon to determine the correct subscripts in the formula.