Calculate the mass, in kg, in each sample. Express your answer with the appropriate UNITS a.) 9.64 x 10^26 cadmium atoms b.) 2.53 x 10^27 nickel atoms c.) 9.33 x 10^27 manganese atoms d.) 3.25 x 10^29 lithium atoms
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Step 1
Number of moles = \( \frac{9.64 \times 10^{26}}{6.022 \times 10^{23}} \) Number of moles = 159.879 Mass = 159.879 x 112 g Mass = 17907.348 g Mass = 17.907348 kg Show more…
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Calculate the mass, in $\mathrm{kg},$ of each sample. $$\begin{array}{l}{\text { a. } 7.55 \times 10^{26} \text { cadmium atoms }} \\ {\text { b. } 8.15 \times 10^{27} \text { nickel atoms }} \\ {\text { c. } 1.22 \times 10^{27} \text { manganese atoms }} \\ {\text { d. } 5.48 \times 10^{29} \text { lithium atoms }}\end{array}$$
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