Stoichiometry Problem........please help

Silver Nitrate reacts with calcium chloride according to the following reaction:

2 AgNO3 (aq) + CaCl2(aq) -- > 2 AgCl(s) + Ca(NO3)2 (aq)

Calculate the mass of AgCl that would be formed by reacting 100 cm3 of 0.200 M AgNO3 solution with 100cm3 of 0.500 M CaCl2 solution. Which of the two solutions is the limiting reagent? What will be the concentration of the solution that is in excess?

Please help.......

1 Answers

Saumil Sachdeva ·

2 AgNO3 (aq) + CaCl2(aq) -- > 2 AgCl(s) + Ca(NO3)2 (aq)

moles of AgNO3 = Molarity x Volume(in L)
=0.2 x 0.1
=0.02 moles

moles of CaCl2 = 0.05 moles

Now by ratio of moles and stoichiometric coefficient we see that (0.02/2) <(0.05/1) .......
Therefore AgNO3 is limiting reagent.

By stoichiometry, moles of AgCl = [(2/2) x 0.02]

Therefore.....mass of AgCl = 0.02 x (108+2x35.5)
=3.58 gram

Concentration of solution that is in excess is given in the question =0.5 M (as CaCl2 is in excess)

(I hope it's correct)

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