Answer
\[\underline{6.25\times {{10}^{18}}}\] excess electrons and \[\underline{5.69\times {{10}^{-9}}\text{ g}}\]
Work Step by Step
The electronic charge is \[-1.6\times {{10}^{-19}}\text{ C}\]. Calculate the number of electrons as follows:
\[\begin{align}
& \text{Number of electrons}=\frac{\left( -1.0\text{ C} \right)}{-1.6\times {{10}^{-19}}\text{ C}} \\
& =6.25\times {{10}^{18}}
\end{align}\]
The electron has a mass of \[9.10\times {{10}^{-28}}\text{ g}\]. Calculate the total mass as follows:
\[\begin{align}
& \text{Mass}=\left( 6.25\times {{10}^{18}} \right)\left( 9.10\times {{10}^{-28}}\text{ g} \right) \\
& =5.\text{69}\times \text{1}{{\text{0}}^{-9}}\text{ g}
\end{align}\]
The number of electrons necessary is \[\underline{6.25\times {{10}^{18}}}\] and the collective mass is \[\underline{5.69\times {{10}^{-9}}\text{ g}}\].
