Calculate the empirical formula for the compound
1.245g Ni, 5.381g I
Can you help with the steps please
Of course! To find the empirical formula for a compound, you need to determine the relative number of atoms of each element present in the compound. Here are the steps to calculate the empirical formula using the given weights of nickel (Ni) and iodine (I):
Step 1: Convert the given masses into moles.
To do this, divide each given mass by the molar mass of the respective element. The molar mass of nickel (Ni) is 58.69 g/mol, and the molar mass of iodine (I) is 126.90 g/mol.
- Moles of Ni = 1.245g Ni / 58.69 g/mol = 0.0212 mol Ni
- Moles of I = 5.381g I / 126.90 g/mol = 0.0424 mol I
Step 2: Determine the mole ratio.
Divide each mole value by the smallest mole value to get the mole ratio of the elements.
In this case, the smallest mole value is 0.0212 mol Ni.
- Mole ratio of Ni = 0.0212 mol Ni / 0.0212 mol = 1
- Mole ratio of I = 0.0424 mol I / 0.0212 mol = 2
Step 3: Write the empirical formula.
Use the mole ratios determined in step 2 to write the empirical formula. The empirical formula shows the simplest whole number ratio of atoms.
- Empirical formula = NiI2
Therefore, the empirical formula for the compound with 1.245g Ni and 5.381g I is NiI2.