Balance the following equation, using simplest, whole number coefficients. Then answer the following by using the balanced equation, considering each part independent of one another.
___ Zn(s) + ___ Pb(NO3)4 (aq) --> ___ Pb(s) + ___ Zn (NO3) 2 (aq)
a) How many moles of zinc would be needed to yield 7.25 moles of zinc nitrate?
b) how many grams of lead(IV) nitrate will produce 1.47g of zinc nitrate ?
c) What mass of lead would be formed when 75.0g of Zn and 25.0g of Pb(NO3)4 are reacted? Identify the limiting and excess reactant (by formula).
limiting reactant _______________ excess reactant____________________
If the reaction in part C above was performed in the lab with those starting quantities of reactants and ended up with an 81 % yield, how much Pb was actually isolated in the lab?
Balance the following equation, using simplest, whole number coefficients. Then answer the following by using the balanced equation, considering each part independent of one another.
___ Zn(s) + ___ Pb(NO3)4 (aq) --> ___ Pb(s) + ___ Zn (NO3) 2 (aq)
a) How many moles of zinc would be needed to yield 7.25 moles of zinc nitrate?
b) how many grams of lead(IV) nitrate will produce 1.47g of zinc nitrate ?
c) What mass of lead would be formed when 75.0g of Zn and 25.0g of Pb(NO3)4 are reacted? Identify the limiting and excess reactant (by formula).
limiting reactant _______________ excess reactant____________________
If the reaction in part C above was performed in the lab with those starting quantities of reactants and ended up with an 81 % yield, how much Pb was actually isolated in the lab?
Related textbook solutions
Basic Chemistry
Principles of Chemistry Molecular Approach
Chemistry: Structure and Properties
Principles of Chemistry Molecular Approach
Chemistry: A Molecular Approach
Chemistry: A Molecular Approach
Principles of Chemistry: A Molecular Approach
