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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.

  • CHEM -

    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.

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