Asked by layla
For each of the reactions, calculate the mass (in grams) of the product formed when 15.81 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.
2K(s)+Cl2(g)––––––→2KCl(s)
2K(s)+Cl2(g)––––––→2KCl(s)
Answers
Answered by
oobleck
so, which is underlined?
convert grams to moles
the equation tells you how many moles of product to expect
convert that to grams
convert grams to moles
the equation tells you how many moles of product to expect
convert that to grams
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