Interpreting Chemical Reaction Equations
The 4 reaction assumptions
1. Reactions are spontaneous
2. Reactions are fast
3. Reactions are quantitative
4. Reactions ae stoichiometric
According to the following equation,
CH3OH(l) + CO(g) --> CH3COOH(l)
Calculate the mass of ethanoic acid that would be produced by the reaction of 6.0 x 104 g of carbon monoxide gas with methanol.
mCH3COOH(l) = 1.3 x 105 g
What is the volume of 2.0 mol of chorine gas at 75 kPa and 27 °C ?
67 L
The last step in manufacturing nitric acid, HNO3(aq), involves this reaction:
3NO2(g) + H2O(l) --> 2HNO3(aq) + NO(g)
What volume of 15.4 mol/L HNO3(aq) is prepared from the reaction of 2.31 x 104 mol of NO2(g)?
1.00 x 103 L
The difference between % yield and % error
% yield tells you how efficient a reaction is.
% error tells you how accurate your results are to the theoretical values.
In the form abcd, where a is the coefficient of the first reactant, b is the coefficient of the second reactant, c is the coefficient of the first product, and d is the coefficient of the second product, balance the following chemical reaction:
Ba(ClO3)2(aq) + Na3PO4(aq) --> Ba3(PO4)2(s) + NaClO3(aq)
3216
As an experiment, a student performed a single-replacement reaction by dipping a strip of copper metal into an aqueous solution of silver nitrate to produce silver.
Calculate the mass of silver that would be produced if the copper strip had a mass of 1.00 g.
mAg(s) = 3.39 g
What volume of NO(g) can be produced when 450.0 L of NO2(g) react at 22.15 °C and 500 kPa pressure according to the reaction
3NO2(g) + H2O(l) --> 2HNO3(aq) + NO(g)
150.0 L
Sulfuric acid can be neutralized by reacting it with aqueous barium hydroxide. What volume of of 0.676 mol/L H2SO4(aq) can be neutralized by 22.7 mL of 0.385 mol/L Ba(OH)2(aq)?
VH2SO4(aq) = 12.9 mL
100.0 mL f 0.200 mol/L HBrO3(aq) is reacted with SO2(g). Calculate the percentage error if 3.55 g of H2SO4(aq) is produced.
2HBrO3(aq) + 5SO2(g) + 4H2O(l) --> Br2(g) + 5H2SO4(aq)
27.6%
Write the net ionic equation for the following balanced reaction:
2Al(s) + 3CuCl2(aq) --> 3Cu(s) + 2AlCl3(aq)
2Al(s) + 3Cu+(aq) --> 3Cu(s) + 2Al3+(aq)
Calculate the mass of liquid metal element produced by the decomposition of a 23.3 g mass of mercury (II) sulfide.
m = 20.1 g
Oxygen gas and magnesium react to form 2.43 g of magnesium oxide. What volume of oxygen gas at SATP would be consumed to produce this mass of MgO(s)?
0.748 L
Hydrochloric acid reacts with pure magnesium carbonate according to the balanced chemical equation:
MgCO3(s) + 2HCl(aq) --> MgCl2(aq) + H2O(l) + CO2(g)
What volume of 0.383 mol/L hydrochloric acid is needed to react with 1.62 g of pure magnesium carbonate?
0.100 L
100.0 mL f 0.200 mol/L HBrO3(aq) is reacted with SO2(g). Calculate the percentage yield if 3.55 g of H2SO4(aq) is produced.
2HBrO3(aq) + 5SO2(g) + 4H2O(l) --> Br2(g) + 5H2SO4(aq)
72.4 %
In a hard water analysis, sodium oxalate solution reacts with calcium hydrogen carbonate present in the hard water to precipitate a calcium compound. Write the net ionic equation for this reaction.
Ca2+(aq) + C2O42-(aq) -> CaC2O4(s)
The exhaled carbon dioxide, CO2(g) produced by astronauts can be removed using lithium hydroxide, LiOH(s). The reaction produces lithium carbonate and water. An astronaut exhales an average of 1.00 x 103 g of carbon dioxide each day. What mass of lithium hydroxide should engineers place on board a spacecraft, per astronaut, per day?
mLiOH(s) = 1.09 x 103 g
What is the concentration of HNO3(aq) if 50.8 mL of 0.0800 mol/L NaOH(aq) neutralize 30.0 mL of the acid?
0.135 mol/L HNO3(aq)
When solutions of lead (II) nitrate and sodium iodide are mixed, a bright yellow precipitate appears. What volume of 0.125 mol/L NaI(aq) is necessary to precipitate all the aqueous lead (II) ions in 25.0 mL of 0.100 mol/L Pb(NO3)2(aq)?
40.0 mL
Calculate the percentage yield for the following reaction if 60 g of SO2(s) is produced using 50 g of S8(s)
S8(s) + 8O2(g) --> 8SO2(s)
60%