Final answer:
To find the grams of barium nitrate in a 2.5 mole sample, we calculate the molar mass of barium nitrate and multiply it by the number of moles, resulting in 653.3425 grams of barium nitrate.
Step-by-step explanation:
The question asks how many grams of barium nitrate, Ba(NO3)2, are in a 2.5 mole sample. To find the answer, let's first calculate the molar mass of barium nitrate. Here are the steps involved:
- Determine the atomic masses: barium (Ba) has an atomic mass of 137.327 g/mol, nitrogen (N) has an atomic mass of 14.007 g/mol, and oxygen (O) has an atomic mass of 15.999 g/mol.
- Calculate the total molar mass: molar mass of Ba(NO3)2 = (1 x 137.327) + (2 x (1 x 14.007) + (3 x 15.999)) = 137.327 + 2 x (14.007 + 3 x 15.999) = 137.327 + 164.09 = 261.337 g/mol.
- Multiply the molar mass by the number of moles: 261.337 g/mol x 2.5 moles = 653.3425 grams.
Therefore, a 2.5 mole sample of barium nitrate contains 653.3425 grams.