# Answer to Question #57158 in General Chemistry for nicki

Question #57158

given that the dominant isotope mass for copper metal is 62.94 amu (g/mol) how many atoms of copper metal are in a pure copper coin that weighs 2.15g

Expert's answer

n(Cu) = 2.15 / 62.94 = 0.0342 (mol);

N(Cu) = 0.0342 * 6.02 *1023 = 2.06 *1022

Answer: 2.06 *1022 atoms

N(Cu) = 0.0342 * 6.02 *1023 = 2.06 *1022

Answer: 2.06 *1022 atoms

Need a fast expert's response?

Submit orderand get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

## Comments

## Leave a comment