Asked by K
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.
2K(s) + __Cl2(g)__ -> 2KCl(s)
I cannot get the correct answer.
2K(s) + __Cl2(g)__ -> 2KCl(s)
I cannot get the correct answer.
Answers
Answered by
bobpursley
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.
That number, times two, is the number of moles of KCl. Change that amount of moles to grams of KCl.