Chemistry Help

posted by Kelly

I have tried usingg the molecular formula, formulas in the text book but my answers dosent match any of the multiple choice answers, can someone help?

For each of the reactions shown, calculate the mass (in grams) of the product formed when 10.7 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

2K(s)+Cl_2(g) ->2K Cl(s)

2K(s)+ Br_2(l) -> 2KBr(s)

  1. DrBob222

    moles Cl2 = 10.7/about 71 = about 0.15
    Convert moles Cl2 to moles KCl.
    0.15 moles Cl2 x (2moles KCl/1 mole Cl2) = 0.15 x (2/1) = 0.30 moles.
    g KCl = moles x molar mass. = about 0.30 x 74.55 = about 22.5 grams KCl.
    You must go through and calculate more precisely than I. Be careful with the number of significant figures.
    I obtained an exact value of
    22.501 which will round to 22.5 grams to three s.f.
    The KBr problem is done the same way. My number for that problem is
    15.935 grams which rounds to 15.9 g to three s.f.

  2. Kelly

    Thank you so much for your help, for the following question i am getting wrong answers answell. for the first one i got 42.7 and the 2nd I got 19.8. Could you help? Thank you for help in advance

    4Cr(s) = 3O_2(g) -> 2Cr_2O_3(s)


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