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) Responses The student calculated the correct number of molecules of ammonium acetate. The student calculated the correct number of molecules of ammonium acetate. The student miscalculated the number of molecules of ammonium acetate.

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) Responses The student calculated the correct number of molecules of ammonium acetate. The student calculated the correct number of molecules of ammonium acetate. The student miscalculated the number of molecules of ammonium acetate.

Answer 1

The student miscalculated the number of molecules of ammonium acetate.

To calculate the correct number of molecules of ammonium acetate used in the reaction, we need to use Avogadro's number, which is 6.022×10^23 molecules/mol.

So, the correct calculation would be:
(0.100 mol) x (6.022×10^23 molecules/mol) = 6.022×10^22 molecules

Therefore, the correct number of molecules of ammonium acetate used in the reaction is 6.022×10^22 molecules, not 4.64×10^24 molecules as calculated by the student.