What quantities are conserved in chemical reactions?

grams and atoms

What quantities are not conserved in chemical reactions?

liters and moles

When calculating percent yield, actual yield and theoretical yield are always ____________ of the same ____________.

grams, product

How many moles of Ca(OH)2

are needed to react completely with 2.35 moles of Al2(SO4)3 according to the following balanced chemical reaction?

7.05 moles Ca(OH)2

AlAl22(SO(SO44))33 + 3Ca(OH) + 3Ca(OH)22 2Al(OH) 2Al(OH)33 + 3CaSO + 3CaSO44

Using the following balanced equation, calculate the number of grams of water formed when 0.75 moles of B(OH)3 are used in the reaction.

40.54 g H2O

3 H3 H22SOSO44 + 2 B(OH) + 2 B(OH)33 B B22(SO(SO44))33 + + 6H6H22OO

How many moles of MgO form from the reaction below if enough reactants are used to form 15.98 g of Fe?

0.43 mol MgO

3 Mg + Fe3 Mg + Fe22OO33 2 Fe + 3 MgO 2 Fe + 3 MgO

Using the following equation:Pb(SO4)2 + 4 LiNO3 Pb(NO3)4 + 2 Li2SO4 

How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?

313.58 g LiNO3

How many liters of NH3 at STP form when 15.23 g of ammonium carbonate, (NH4)2CO3, decompose according the following balanced equation?

(NH4)2CO3 H2O + 2NH3 + CO2

7.10 L NH3

Calcium carbonate decomposes to form carbon dioxide and calcium oxide: CaCO3 (s) CO2(g) + CaO(s)How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide at STP?

15.42 g

Ethylene burns in oxygen to form carbon dioxide and water vapor: C2H4(g) + 3 O2(g) 2 CO2(g) + 2 H2O(g)

How many liters of water vapor can be formed if 1.25 liters of ethylene are consumed in this reaction? Assume all substances are at the same temperature and pressure.

2.50 L H2O

Calculate the following: a) Which of the reagents is the limiting reagent?b) How many grams of each product are formed?c) How many grams of excess reactant remain? 3 NH4NO3 + Na3PO4 (NH4)3PO4 + 3 NaNO3

Assume we started with 30 grams of ammonium nitrate and 50 grams of sodium phosphate.

a) ammonium nitrate

b) 18.6 grams of ammonium phosphate, 31.9 grams of sodium nitrate

c) 29.5 grams of sodium phosphate

If the percent yield of the following equation is 55%, how many grams of H2SO4 are produced when 44.8 L of SO3 are combined with excess water? Assume the reaction occurs at STP. SO3(g) + H2O(l)→H2SO4(aq)

107.89 g H2SO4

A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen.  Which is the limiting reactant and how many grams of excess reactant remains after the reaction has stopped? 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)

oxygen, 0.30 g NH3

90.0 g of FeCl3 reacts with 52.0 g of H2S, according to the following balanced equation:2FeCl3 + 3H2S Fe2S3 + 6HCl What is the limiting reactant?  What is the mass of HCl produced?  What mass of excess reactant remains after the reaction?

FeCl3, 60.8 g HCl, 23.6 g H2S

If 12.0 mL of 1.34 M NaOH is required to neutralize 25.00 mL of a sulfuric acid, H2SO4, solution, what is the molarity of the sulfuric acid?The balanced titration reaction is H2SO4(aq) + 2NaOH(aq) Na2SO4(aq) + 2HOH(l).

0.322 M H2SO4

What volume (in mL) of 0.075 M HCl is required to neutralize 100 mL of 0.01 M Ca(OH)2 solution? The balanced titration reaction is2HCl + Ca(OH)2 2H2O + CaCl2.

26.7 mL HCl