Balancing Rxns & Ionic Equations
Acid/Base &
Oxidation/Reduction
Oxidation/Reduction
Enthalpy & Energy
Stoich, Theoretical & Percent Yield
100
Balance the following rxn and determine the type of rxn:
Cu(OH)2 + HC2H3O2 → Cu(C2H3O2)2 + H2O
Cu(OH)2 + 2HC2H3O2 → Cu(C2H3O2)2 + 2H2O
double replacement
100
List the oxidation #s for all atoms in the following:
Pb(NO3)2
Pb: +2
O: -2
N: +5
100
-triangle H = ? rxn, ? heat
triangle H = ? rxn, ? heat
exothermic, releases heat
endothermic, absorbs heat
100
A chemist performs a synthesis where the calculated theoretical yield of a compound is 55g. After completing the experiment, they isolate 44.0g of the product. What is the percent yield?
80%
200
The reaction of the organic compound, C3H8O with oxygen gas to form products. Write the balanced rxn
2C3H8O + 9O2(g) --> 6CO2(g) + 8H2O(l)
200
False, oxidation #s did not change
200
How many kilojoules of heat are produced by the reaction of 25.0 g of water?
Mg(s) + 2 H2O(l) → Mg(OH)2(s) + H2(g)
ΔHrxn = −353 kJ
245 kJ
200
How many moles of water can we make from 6 moles of hydrogen and 4 moles of oxygen?
2 H2(g) + O2(g) → 2H2O(g)
6 mol H2O
300
Write the following rxn, balance it and determine if the compounds are soluble
aqueous potassium sulfate is mixed with aqueous barium bromide
K2SO4 (aq) + BaBr2 (aq) -->2KBr(aq) + BaSO4 (s)
300
Balance the following rxn and label the acid and base:
HF + Ba(OH)2 --> H2O + BaF2
2HF + Ba(OH)2 --> 2H2O + BaF2
acid base
300
If you have 9.0 kg of C3H8, how many kilojoules of energy did you generate?
C3H8(l) + 5O2(g) → 3CO2(g) + 4H2O(l)
ΔHrxn = −2219.1 kJ
And how many pounds of carbon dioxide did you release into the atmosphere?
4.5x105 kJ
59 lb of CO2
300
What volume, in liters, of 0.150 M BaCl2 solution is needed to react completely with 0.200 L of a 0.450 M AgC2H3O2 solution according to the equation:
BaCl2(aq) + 2AgC2H3O2(aq) → Ba(C2H3O2)2(aq) + 2AgCl(s)
0.3 L
400
Write the balanced full chemical equation, complete ionic equation, and net ionic equation for the reaction between calcium sulfide and ammonium phosphate. Be sure to include physical states.
Full:
3CaS(aq) + 2(NH4)3PO4(aq) → Ca3(PO4)2(s) + 3(NH4)2S(aq)
Complete Ionic:
3Ca2+(aq) + 3S2−(aq) + 6NH4+(aq) + 2PO43−(aq) → Ca3(PO4)2(s) + 6NH4+(aq) + 3S2−(aq)
Net Ionic:
3Ca2+(aq) + 2PO43−(aq) → Ca3(PO4)2(s)
400
Finish the following rxn, balance it, and indicate the conjugate acid & conjugate base
H2CO3 +Sr(OH)2 -->
H2CO3 + Sr(OH)2 --> SrCO3 + 2H2O
400
How many grams of ammonia and oxygen are required to produce 2,500 kJ of energy?
4 NH3(l) + 5 O2(aq) → 4 NO(g) + 6 H2O(l) ΔHrxn = −1,170 kJ
150g NH3
430g O2
400
Calculate the maximum number of grams of NH3 that can be produced by the reaction of 2.00 g of N2 with 3.00 g H2. Also determine the percent yield if the experiment yields 2.17g of NH3.
N2(g) + 3 H2(g) → 2 NH3(g)
LR = N2
Theoretical yield =2.43g
Percent Yield = 89.3%
500
Write the balanced full chemical equation, complete ionic equation, and net ionic equation for the reaction between molybdenum(V) iodide and potassium carbonate. Be sure to include physical states.
Full chemical eq: 2MoI5(aq) + 5K2CO3(aq) → Mo2(CO3)5(s) + 10KI(aq)
Complete Ionic:
2Mo5+(aq) + 10I−(aq) + 10K+(aq) + 5CO32−(aq) →
Mo2(CO3)5(s) + 10K+(aq) + 10I−(aq)
Net Ionic: 2Mo5+(aq) + 5CO32−(aq) → Mo2(CO3)5(s)
500
Finish the following rxn, balance it, and indicate the conjugate acid & conjugate base:
H3PO4 + Ca(OH)2 --> ?
List the oxidation #s for the elements in the following:
FeCO3
2H3PO4 + 3Ca(OH)2 --> 6H2O + Ca3(PO4)2
Fe: +2
C:+4
O:-2
500
A rocket ship was powered by a propellant made of hydrazine, N2H4, combined with an oxidizer, N2O4, that reacted according to the following equation:
2N2H4(l) + N2O4(l) → 3N2(g) + 4H2O(g) ΔHrxn = −1049 kJ
The average mass of propellant for the rocket ship was 5,187 lb. Assuming it was a 50:50 mixture, what’s the maximum amount of heat it could produce?
1.341×107 kJ of heat produced
500
When iron metal is heated with oxygen gas it produces solid iron(III) oxide. If 50.0 g of iron are reacted with 25.0 g of oxygen, what is the theoretical yield of iron(III) oxide in grams?
When running this experiment in the lab, 49.7 g of iron(III) oxide was produced. What was the percent yield?
Balanced Eq = 4Fe(s) + 3O2(g) → 2Fe2O3(s)
Theoretical Yield = 71.5g
Percent Yield = 69.5%