3. 50.0 mL of 0.500 mol/L copper (II) sulphate solution is mixed with 50.0 mL of 1.00 mol/L sodium hydroxide in a coffee cup calorimeter. The initial temperature of the water is 18.9°C, and the final temperature is 24.0°C. a) Calculate the molar enthalpy change for this reaction per mole of CuSO4. b) Write the thermochemical reaction.
3. 50.0 mL of 0.500 mol/L copper (II) sulphate solution is mixed with 50.0 mL of 1.00 mol/L sodium hydroxide in a coffee cup calorimeter. The initial temperature of the water is 18.9°C, and the final temperature is 24.0°C. a) Calculate the molar enthalpy change for this reaction per mole of CuSO4. b) Write the thermochemical reaction.
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Transcribed Image Text:3. 50.0 mL of 0.500 mol/L copper (II) sulphate solution is mixed with 50.0 mL of 1.00 mol/L sodium hydroxide in a
coffee cup calorimeter. The initial temperature of the water is 18.9°C, and the final temperature is 24.0°C.
a) Calculate the molar enthalpy change for this reaction per mole of CuSO4.
b) Write the thermochemical reaction.
Transcribed Image Text:Selected Standard Molar Enthalpies of Formation
AH₁
AH;
AH₁
Substance (kJ/mol) Substance (kJ/mol) Substance (kJ/mol)
Al₂O3(s)
-1675.7 HBr(g)
CaCO3(s)
-1207,6 HCl(g)
CaCl₂(s)
Ca(OH)₂(s)
CCL₂(E)
CCL4(8)
CHCI ()
CH₂(g)
C₂H₂(g)
C₂H₁(g)
C₂H₂(g)
CzHs(g)
CH()
CH₂OH(E)
C₂H₂OH()
CO(g)
CO₂(g)
COCI₂(g)
+49.1 Fe₂O₂(8)
-239.2 Fe,O4(s)
-277.6 FeCl₂(s)
CH3COOH(E) –484.3 FeCls(s)
-110.5 FeS (8)
CS₂(e)
CS₂(g)
CrCla(g)
Cu(NO₂)₂ (8)
-795.4 HF(g)
-985.2 HCN(g).
-128.2 H₂O(E)
-95.7 H₂O(g)
CuO(s)
CuCl(s)
CuCl₂(s)
-134.1 H₂O₂(e)
-74.6 HNO (0)
+227.4 H₂PO4(s)
+52.4 H₂S(g)
-84.0 H₂SO4(e)
-103.8 FeO(s)
–36.3|NH(8)
-92.3 N₂H4(e)
-273.3 NH Cl(s)
+135.1 NH₂NO(s)
-285.8 NO(g)
-393.5 PbCl₂(s)
-219.1 MgCl₂(s)
+89.0 MgO(s)
+116.7 Mg(OH)2(s)
-556.5 HgS(s)
-241.8 NO₂(g)
-187.8 N₂O(g)
-174.1 N₂O(g)
1284.4 PH,(g)
-20.6 PCl₂(g)
814.0 P,O,(s)
-272.0 P4O₁0(s)
-824.2 KBr(s)
-1118.4 KCl(s)
-341.8 KCIO,(s)
-399.5 KOH(s)
-178.2 AgaCO₂ (s)
-359.4 AgCl(s)
-641.3 AgNO,(s)
-601.6 Ag S(s)
-924.5 SFB(g)
-58.2 SO₂(g)
-302.9 NaCl(s)
-411.2 SO₂(g)
-157.3 NaOH(s)
-425.6 SnCl₂(s)
-137.2 Na₂CO3(s)-1130.7 SnCl4(e)
-220.1
-45.9
+50.6
-314.4
-365.6
+91.3
+33.2
+81.6
+11.1
+5.4
-287.0
-2144.3
-2984.0
-393.8
-436.5
-397.7
-424.6
-505.8
-127.0
-124.4
-32.6
-1220.5
-296.8
-395.7
-325.1
-511.3
Note: The enthalpy of formation of an element in its standard state is
defined as zero.
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