The molar mass of ammonium acetate is 77.083 g/mol. A student uses 0.100 mol of ammonium acetate in a chemical reaction. The student claims that the reaction uses (0.100 mol)(77.083 gmol) = 7.71 g of ammonium acetate, which has (7.71)(6.022×1023) = 4.64×1024 molecules. Did the student determine the correct number of molecules of ammonium acetate used in the reaction? (2 points)

Question

The molar mass of ammonium acetate is 77.083 g/mol. A student uses 0.100 mol of ammonium acetate in a chemical reaction. The student claims that the reaction uses (0.100 mol)(77.083 gmol) = 7.71 g of ammonium acetate, which has (7.71)(6.022×1023) = 4.64×1024 molecules. Did the student determine the correct number of molecules of ammonium acetate used in the reaction? (2 points)

Answer 1

No, the student did not determine the correct number of molecules of ammonium acetate used in the reaction. To calculate the number of molecules of a substance, you need to use Avogadro's number, which is 6.022×10^23 molecules/mol.

Therefore, if the student used 0.100 mol of ammonium acetate, the correct number of molecules used in the reaction would be:

0.100 mol x 6.022×10^23 molecules/mol = 6.022×10^22 molecules

So, the correct number of molecules of ammonium acetate used in the reaction is 6.022×10^22 molecules, not 4.64×10^24 molecules.