Final answer:
To prepare 600 mL of a 2.2 M solution of calcium nitride, we calculate the molar mass of the compound, determine the number of moles required using the solution's molarity, and then calculate the mass, which is 232.647 grams.
Step-by-step explanation:
To calculate the mass of calcium nitride (Ca3N2) required to make 600 mL of a 2.2 M solution, first we need to find the molar mass of calcium nitride. We do this by multiplying the atomic masses of calcium (Ca) and nitrogen (N) by the number of atoms in the formula Ca3N2:
- 3 x 40.078 g/mol for calcium
- 2 x 14.007 g/mol for nitrogen
Adding these together gives us:
3 x 40.078 g/mol + 2 x 14.007 g/mol = 148.234 g/mol for Ca + 28.014 g/mol for N = 176.248 g/mol for Ca3N2
Next, we use the volume and molarity to find the number of moles of calcium nitride needed:
600 mL is 0.6 L (since there are 1000 mL in a liter). At a concentration of 2.2 M (moles per liter), we need 0.6 L x 2.2 mol/L = 1.32 moles of Ca3N2.
Finally, we calculate the mass:
1.32 moles x 176.248 g/mol = 232.647 grams of calcium nitride.