Gas Law Review
• Ex. 1: A sample of O2 gas initially present in a
2.00 L container at a pressure of 2.40 atm and
22 oC is moved to a 5.00 L container at 15 OC.
A sample of Ne gas initially held at a pressure
of 4.00 atm and -16 OC in a 4.00 L container is
added to the oxygen gas in the 5.00 L
container (still at 15 OC). What is the total
pressure in the 5.00 L container?
Stoichiometry Review
• Ex. 2: Aqueous potassium dichromate,
K2Cr2O7(aq), can oxidize ethanol to acetic acid in
the presence of excess sulfuric acid The net ionic
equation for this reaction is
• 2 Cr2O72-(aq) + 3 CH3CH2OH(aq) + 16 H+(aq) →
3 CH3COOH(aq) + 4 Cr3+(aq) + 11 H2O(l)
• (a) Identify the limiting reagent if 3.50 mL of pure
ethanol, CH3CH2OH(l), are mixed with 48.0 mL
of 1.00 mol.L-1 K2Cr2O7(aq) and excess acid. The
density of pure ethanol is 0.789 g.mL-1.
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Stoichiometry Review
• (b) What is the theoretical yield of acetic acid
in moles and in grams?
• (c) What is the % yield of acetic acid if 2.89 g
of CH3COOH(l) was obtained after the product
mixture had been purified?
Stoichiometry Review
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Other stoichiometric complications:
1. Impure starting materials.
2. Starting material is a mixture.
3. Gaseous products or reactants.
4. Gases collected over water.
Calorimetry Review
• Ex. 3 A 5.00 mL volume of a 0.60 M solution of
phosphoric acid, H3PO4(aq), reacts with 45.00 mL of
0.25 M NaOH(aq) according to the reaction below. The
temperature of the solution rises from 22.5 oC to 24.5
oC. Assuming the volumes of the solutions are additive,
and the density of the final solution is 1.10 g mL–1,
calculate the enthalpy change for the reaction. Assume
the heat capacity of the solution is the same as water
and the water produced by the reaction does not affect
the volume of the resulting solution.
• H3PO4(aq) + 3 NaOH(aq)  Na3PO4(aq) + 3 H2O(l)
Hrxn = ?
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Calorimetry Review
• Ex. 4:Nitrous oxide, N2O(g), reacts with carbon
disulfide, CS2(g) according to the equation below.
When performed in a constant volume bomb
calorimeter with a heat capacity of 8.775 kJ ºC–1,
the temperature of the calorimeter rises from
22.53 ºC to 29.13 ºC and forms 2.48 g of sulfur,
S(s). Determine the internal energy change, ∆U,
and the enthalpy change, ∆H of the following
reaction at 25.0 °C.
• 3 N2O(g) + CS2(l)  3 N2(g) + CO(g) + S(s)