If 100.0 mL100.0 mL of 0.361 M Na2SO40.361 M Na2SO4 is added to 100.0 mL100.0 mL of 0.881 M Pb(NO3)20.881 M Pb(NO3)2 , how many grams of PbSO4PbSO4 can be produced? Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s)Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s) STRATEGY Calculate the initial moles present and add them to a table of initial, change, and end of reaction moles. Determine the limiting reactant using the comparison of moles method. Use the limiting reactant to determine the change in moles for each reactant and product, then complete the table of moles. Convert the moles of PbSO4PbSO4 produced to the mass of PbSO4PbSO4 , in grams. Step 1: Calculate the initial moles of Na2SO4Na2SO4 and Pb(NO3)2Pb(NO3)2 present and add them to the table. Na2SO4(aq)Na2SO4(aq) ++ Pb(NO3)2(aq)Pb(NO3)2(aq) ⟶⟶ 2NaNO3(aq)2NaNO3(aq) ++ PbSO4(s)PbSO4(s) initial moles ? ? 0 0 change in moles end moles initial moles of Na2SO4Na2SO4 : initial moles of Pb(NO3)2Pb(NO3)2 :
If 100.0 mL100.0 mL of 0.361 M Na2SO40.361 M Na2SO4 is added to 100.0 mL100.0 mL of 0.881 M Pb(NO3)20.881 M Pb(NO3)2 , how many grams of PbSO4PbSO4 can be produced? Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s)Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s) STRATEGY Calculate the initial moles present and add them to a table of initial, change, and end of reaction moles. Determine the limiting reactant using the comparison of moles method. Use the limiting reactant to determine the change in moles for each reactant and product, then complete the table of moles. Convert the moles of PbSO4PbSO4 produced to the mass of PbSO4PbSO4 , in grams. Step 1: Calculate the initial moles of Na2SO4Na2SO4 and Pb(NO3)2Pb(NO3)2 present and add them to the table. Na2SO4(aq)Na2SO4(aq) ++ Pb(NO3)2(aq)Pb(NO3)2(aq) ⟶⟶ 2NaNO3(aq)2NaNO3(aq) ++ PbSO4(s)PbSO4(s) initial moles ? ? 0 0 change in moles end moles initial moles of Na2SO4Na2SO4 : initial moles of Pb(NO3)2Pb(NO3)2 :
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter13: The Chemistry Of Solutes And Solutions
Section: Chapter Questions
Problem 137QRT
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Question
If 100.0 mL100.0 mL of 0.361 M Na2SO40.361 M Na2SO4 is added to 100.0 mL100.0 mL of 0.881 M Pb(NO3)20.881 M Pb(NO3)2 , how many grams of PbSO4PbSO4 can be produced?
Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s)Na2SO4(aq)+Pb(NO3)2(aq)⟶2NaNO3(aq)+PbSO4(s)
STRATEGY
-
Calculate the initial moles present and add them to a table of initial, change, and end of reaction moles.
-
Determine the limiting reactant using the comparison of moles method.
-
Use the limiting reactant to determine the change in moles for each reactant and product, then complete the table of moles.
-
Convert the moles of PbSO4PbSO4 produced to the mass of PbSO4PbSO4 , in grams.
Step 1: Calculate the initial moles of Na2SO4Na2SO4 and Pb(NO3)2Pb(NO3)2 present and add them to the table.
Na2SO4(aq)Na2SO4(aq) | ++ | Pb(NO3)2(aq)Pb(NO3)2(aq) | ⟶⟶ | 2NaNO3(aq)2NaNO3(aq) | ++ | PbSO4(s)PbSO4(s) | |
---|---|---|---|---|---|---|---|
initial moles | ? | ? | 0 | 0 | |||
change in moles | |||||||
end moles |
initial moles of Na2SO4Na2SO4 :
initial moles of Pb(NO3)2Pb(NO3)2 :
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