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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
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