Balance and complete each of the following, and indicate how many moles of the s

Question

Balance and complete each of the following, and indicate how many moles of the second reactant would be required to react completely with 0.150 mol of the first reactant. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer.)

(a) BaCl2(aq) + H2SO4(aq)

(b) AgNO3(aq) + NaCl(aq)

(c) Pb(NO3)2(aq) + Na2CO3(aq)

(d) C3H8(g) + O2(g)

(e) Before going to lab, a student read in his lab manual that the percent yield for a difficult reaction to be studied was likely to be only 20.% of the theoretical yield. The student's prelab stoichiometric calculations predict that the theoretical yield should be 11.3 g. What is the student's actual yield likely to be?

(f) According to his prelaboratory theoretical yield calculations, a student's experiment should have produced 1.67 g of magnesium oxide. When he weighed his product after reaction, only 1.11 g of magnesium oxide was present. What is the student's percent yield?

Explanation / Answer

a) BaCl2(aq) + H2SO4(aq) --------> BaSO4(s) + 2HCl(aq)

1 mol of BaCl2 reacts with 1 mol of H2SO4 according to the balanced reaction, so 0.15mol of BaCl2 will react with 0.15mol of H2SO4.

b) AgNO3(aq) + NaCl(aq) --------> AgCl(s) + NaNO3(aq

1 mol of AgNO3 reacts with 1 mol of NaCl according to the balanced reaction, so 0.15mol of AgNO3 will react with 0.15mol of NaCl.

c) Pb(NO3)2(aq) + Na2CO3(aq) -----> PbCO3(s) + 2NaNO3(aq)

1 mol of Pb(NO3)2 reacts with 1 mol of Na2CO3 according to the balanced reaction, so 0.15mol of Pb(NO3)2 will react with 0.15mol of Na2CO3.

d) C3H8(g) + 5O2(g) -----> 3CO2(g) + 4H2O(g)

1 mol of C3H8 reacts with 5 mol of O2, so 0.15mol of C3H8 will react with 0.15x5 ---> 0.75mol O2

e) %yield= actual yield/theoretical yield x 100

20= actual yield/11.3g x 100

actual yield= 2.26g

f) %yield= 1.11/1.67 x 100= 66.5%

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