Give the empirical formula of each of the following compounds ...

Question

Give the empirical formula of each of the following compounds if a sample contains (b) 2.10 g nickel and 0.58 g oxygen

Accepted Answer

Step 1: The first step in determining the empirical formula of a compound is to convert the mass of each element to moles. This is done by dividing the given mass of each element by its atomic mass. The atomic mass of nickel (Ni) is approximately 58.69 g/mol and the atomic mass of oxygen (O) is approximately 16.00 g/mol.. Step 2: After converting the masses to moles, you will have the mole ratio of the elements in the compound. However, this ratio may not be in the simplest whole number form. To find the simplest whole number ratio, divide each value by the smallest number of moles calculated in the previous step.. Step 3: If the mole ratio obtained in the previous step is not a whole number, it may be necessary to multiply each value by a factor (such as 2, 3, etc.) to obtain whole numbers. This is often the case when dealing with elements that tend to form multiple bonds, like oxygen.. Step 4: Once you have the simplest whole number ratio of moles for each element, you can write the empirical formula. The empirical formula is written by listing the elements in the same order as in the original compound formula, followed by the number of atoms of each in subscript (if more than one).. Step 5: It's important to note that the empirical formula does not provide information about the actual number of atoms in a molecule of the compound, it only gives the simplest whole number ratio of atoms. The molecular formula may be a multiple of the empirical formula.

Give the empirical formula of each of the following compounds if a sample contains (b) 2.10 g nickel and 0.58 g oxygen

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Concetti chiave

Empirical Formula

Molar Mass

Stoichiometry