1. The problem statement, all variables and given/known data (a). Calculate the number of electrons in a small, electrically neutral silver pin that has a mass of 10g. Silver has 47 electrons per atom, and its molar mass is 107.87 g/mol. (b). Imagine adding electrons to the pin until the negative charge has the very large value of 1.00 mC. How many electrons are added for every 10^9 electrons already present? 2. The attempt at a solution This problem seems rather simple, but for some reason part b is not making any sense to me... maybe i messed up part a, even though i've checked it through a few times... (a) 10g/107.87(g/mol) = .0927 mol .0927 x (6.022 x 10^23)(avgr #) x 47 electrons, which gives me 2.62 x 10^24 electrons in this 10g of silver. (b). When I multiplied 2.62 x 10^24 (electrons) by -1.602 x 10^-19, which is the charge for a single electron, the final charge i got was 419814.96, which is obviously much larger than 1 mC. Any idea where i went wrong on this old review problem?