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An unknown element M combines with oxygen to form the compound MO2. If 36.0 g of element M combines exactly with 16.00 g of oxygen, what is the molar mass of M in g mol–1?12.072.024.016.0

Question

An unknown element M combines with oxygen to form the compound MO2. If 36.0 g of element M combines exactly with 16.00 g of oxygen, what is the molar mass of M in g mol–1?12.072.024.016.0

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Solution

To solve this problem, we need to use the concept of stoichiometry and the law of conservation of mass. Here are the steps:

  1. First, we need to know the molar mass of oxygen, which is 16.00 g/mol.

  2. From the formula of the compound (MO2), we know that one mole of the unknown element M combines with two moles of oxygen to form one mole of MO2.

  3. According to the problem, 16.00 g of oxygen combines with 36.0 g of the unknown element M. Since the molar mass of oxygen is 16.00 g/mol, this means that 1.00 mol of oxygen combines with 36.0 g of the unknown element M.

  4. However, according to the formula of the compound (MO2), two moles of oxygen combine with one mole of the unknown element M. Therefore, 1.00 mol of the unknown element M would combine with 2 * 16.00 g/mol = 32.00 g of oxygen.

  5. Therefore, the molar mass of the unknown element M is 36.0 g/mol.

This problem has been solved

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