A) \[0.057\times {{10}^{23}}g\]
B) \[2.657\times {{10}^{-23}}g\]
C) \[2.657\times {{10}^{23}}g\]
D) \[4.657\times {{10}^{-23}}g\]
Correct Answer: B
Solution :
Key Idea: Atomic mass = Avogadro number \[6.023\times {{10}^{23}}\] atoms of \[{{O}_{2}}\] is present in = 16 g \[\therefore \] 1 atoms of \[{{O}_{2}}\] is present in \[=\frac{16}{6.023\times {{10}^{23}}}\] \[=2.66\times {{10}^{-23}}g\]
You need to login to perform this action.
You will be redirected in
3 sec
