The chemical formula for zinc nitrate is: \[ \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2} \] Calculate the molar mass of zinc nitrate. Round your answer to 1 decimal place.

To find the molar mass of zinc nitrate \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\), we need to sum the molar masses of each component: - Zinc (Zn): 65.38 g/mol - Nitrogen (N): 14.01 g/mol (there are 2 in the formula) - Oxygen (O): 16.00 g/mol (there are 6 in the formula because of 3 oxygens per nitrate and 2 nitrates) Calculating: 1. Zinc: \( 1 \times 65.38 = 65.38 \, \text{g/mol} \) 2. Nitrogen: \( 2 \times 14.01 = 28.02 \, \text{g/mol} \) 3. Oxygen: \( 6 \times 16.00 = 96.00 \, \text{g/mol} \) Now, add them together: \[ 65.38 + 28.02 + 96.00 = 189.40 \, \text{g/mol} \] Therefore, the molar mass of zinc nitrate, rounded to one decimal place, is \( 189.4 \, \text{g/mol} \).