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 g/mol)=7.71 g

of ammonium acetate, which has (7.71)(6.022×1023)=4.64×1024
molecules.

In one to two sentences, explain the mistake that the student made and determine the correct number of molecules of ammonium acetate used in the reaction.

Answer 1

[AI-generated answer — Bot GPT 3.5]

The student made the mistake of using the molar mass in grams (77.083 g/mol) instead of using the actual amount of ammonium acetate used in the reaction, which is 7.71 g. The correct number of molecules of ammonium acetate used in the reaction would be (7.71 g / 77.083 g/mol) x 6.022x10^23 = 6.04x10^23 molecules.