What is the molar mass of \( \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2} \) ? (Two decimal places, no units)

To calculate the molar mass of \( \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2} \), we need to sum the molar masses of all the atoms in the formula. 1. **Identify the components:** - Iron (Fe): 1 atom - Nitrogen (N): 2 atoms (from \( \mathrm{NO}_{3} \)) - Oxygen (O): 6 atoms (from \( \mathrm{NO}_{3} \), since there are 3 oxygen atoms in each nitrate and there are 2 nitrates) 2. **Molar masses of the elements:** - Molar mass of \( \mathrm{Fe} \) = 55.85 g/mol - Molar mass of \( \mathrm{N} \) = 14.01 g/mol - Molar mass of \( \mathrm{O} \) = 16.00 g/mol 3. **Calculate the total molar mass:** \[ \text{Total Molar Mass} = (1 \times 55.85) + (2 \times 14.01) + (6 \times 16.00) \] Now, let's perform the calculations step by step: - For Iron: \[ 1 \times 55.85 = 55.85 \] - For Nitrogen: \[ 2 \times 14.01 = 28.02 \] - For Oxygen: \[ 6 \times 16.00 = 96.00 \] 4. **Sum the contributions:** \[ \text{Total Molar Mass} = 55.85 + 28.02 + 96.00 \] Now, let's calculate the total: \[ \text{Total Molar Mass} = 55.85 + 28.02 + 96.00 = 179.87 \] Thus, the molar mass of \( \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2} \) is \( 179.87 \). Final answer (to two decimal places, no units): **179.87**.