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Chemistry 1020 Laboratory Manual Winter, 2014 Senior Laboratory Instructor: Richard Bartholomew UA 3071 [email protected] Table of Contents...

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Page number 65. Questons #2-6 please


2. Calculate the ÄH f of the OH ion given that the ÄH f (H2O) = -285.8 kJ mol . 0 - 0 -1

3. In this experiment it was assumed that the calorimeter neither absorbed nor released heat
(i.e., qcalorimeter = 0), but this is almost certainly not the case. Would the measured value of
ÄH rxn for reaction (1.1) be more or less exothermic if the calorimeter absorbed heat (that is, 0
if qcalorimeter > 0)? Explain why.

4. Without doing any calculations, predict whether the observed ÄT would increase, decrease
or remain the same if the following procedural changes were made. Justify your predictions:

a. 50.0 mL of 0.5 mol L-1 NaOH mixed with 50.0 mL of 0.5 mol L-1 HCl.
b. 50.0 mL of 1.0 mol L-1 NaOH + 25.0 mL of water mixed with 25.0 mL of 1.0 mol L-1
HCl.

5. Use tabulated standard molar enthalpy changes of formation (from the textbook) to calculate
ÄH rxn for the following (unbalanced) reactions: 0

a. Al(s) + Fe2O3(s) ÿ Fe(s) + Al2O3(s)
b. PbO(s) + C(s) ÿ CO(g) + Pb(s)
c. CaCO3(s) ÿ CO2(g) + CaO(s)

6. Nitroglycerine is a powerful explosive used for blasting rock in road-making. Ignition
produces water, nitrogen, carbon dioxide and oxygen.
When 200 g of nitroglycerine are detonated 5042 kJ of heat are liberated. Calculate ÄHf for 0
nitroglycerine.
i Chemistry 1020 Laboratory Manual Winter, 2014 Senior Laboratory Instructor: Richard Bartholomew UA 3071 [email protected] Table of Contents DEDICATION. .............................................................. iii LABORATORY ±CALENDAR . .................................................. 1 SAFETY ±RULES. ............................................................. 2 SAFETY ±PROCEDURES . ...................................................... 5 GOOD ±LABORATORY ±PRACTICE . ............................................. 9 LABORATORY ±REPORTS . ................................................... 12 PROCESS FOR RE-SCHEDULING MISSED LABORATORIES . . . . . . . . . . . . . . . . . . . . . . 16 WEIGHING ±TECHNIQUES . ................................................... 18 VOLUMETRIC±TECHNIQUES . ................................................ 22 OPERATION ±OF ±THE ±BUNSEN ±BURNER . ...................................... 29 SUCTION ±FILTRATION . ..................................................... 31 SIGNIFICANT ±FIGURES . ..................................................... 33 LABORATORY ±REPORT ±RECEIPT ±SHEET . ..................................... 39 SAFETY ±ACKNOWLEDGEMENT. ............................................. 40 LOCKER±EQUIPMENT ±LIST . ................................................. 41
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ii 1. THERMOCHEMISTRY AND THE MEASUREMENT OF THE ENTHALPY OF DISSOCIATION ±FOR±ACETIC±ACID. ..................................... 44 2. EFFECT OF CONCENTRATION AND TEMPERATURE ON REACTION RATE . . . . . 67 3 . ± ±pH ±TITRATIONS±AND ±BUFFERS . ........................................... 80 4. DETERMINATION OF THE SOLUBILITY PRODUCT CONSTANT OF CALCIUM HYDROXIDE . ........................................................ 97 5. SYNTHESIS OF MALEIC ACID AND CONVERSION TO FUMARIC ACID. . . . . . . . . 109
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#2) Calculate the ÄH f of the OH ion given that the ÄH f (H2O) = -285.8 kJ mol .
Answer) H+ +
ÄH f OH- H2 O (H+) = 0 ÄH f (OH-) = ?
ÄH f (H2O) = -285.8 kJ mol
ÄH rxn = -57 kJ/mole
ÄH rxn =...

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