Calculate the mass (in grams) of the product formed when 10.1g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

Question

2K(s) + __Cl2(g)__ -> 2KCl(s)

I cannot get the correct answer.

Answer 1

determine how many moles of chlrine 10.1 grams represents.

That number, times two, is the number of moles of KCl. Change that amount of moles to grams of KCl.