A) \[1.032\times {{10}^{22}}\]
B) \[3.01\times {{10}^{22}}\]
C) \[5.88\times {{10}^{23}}\]
D) \[6.023\times {{10}^{23}}\]
Correct Answer: A
Solution :
In 12 g carbon, mass of C-14 isotope \[=12\times \frac{2}{100}=0.24g\] \[\therefore \]Number of C -14 atoms in 12 g of \[C=\frac{0.24}{14}\times 6.02\times {{10}^{23}}\]\[=1.032\times {{10}^{22}}\]
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