A) \[6.023\times {{10}^{19}}\]
B) \[1.084\times {{10}^{18}}\]
C) \[4.84\times {{10}^{17}}\]
D) \[6.023\times {{10}^{23}}\]
Correct Answer: A
Solution :
Density\[=\frac{\text{Mass}}{\text{Volume}}\]; \[1=\frac{g}{ml}\] or \[g=ml\] 0.0018ml = 0.0018gm No. of moles\[=\frac{\text{weight}}{\text{Molecular weight }}=\frac{0.0018}{18}=1\times {{10}^{-4}}\] \[\therefore \] No. of water molecules =\[6.023\times {{10}^{23}}\times 1\times {{10}^{-4}}\] \[=6.023\times {{10}^{19}}\].
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