Issue 1 Iron(III) oxide reacts with carbon monoxide to produce elemental iron and carbon dioxide. Determine the enthalpy change for this reaction using known enthalpies of formation. Fe2O3(s) + 3 CO(g) → 3 CO2(g) + 2 Fe(s)
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.
Issue 1
Iron(III) oxide reacts with carbon monoxide to produce elemental iron and carbon dioxide. Determine the enthalpy change for this reaction using known enthalpies of formation.
Fe2O3(s) + 3 CO(g) → 3 CO2(g) + 2 Fe(s)
Issue 2
Tetraphosphorus decaoxide, P4O10, is an acidic oxide. It reacts with water to produce phosphoric acid, H3PO4, in an exothermic reaction.
P4O10(s) + 6 H2O(l) → 4 H3PO4(aq) ΔHorxn = -257.2 kJ
a) Rewrite the thermochemical equation to include the enthalpy change as a term in the equation.
b) How much energy is released from the reaction of 5.00 mol of P4O10 with excess water?
Issue 4
Find, using Hess's law, the overall enthalpy change of the reaction below. Determine whether the reaction is endothermic or exothermic.
2N2 + 5O2 → 2N2O5
Refer to the following reactions.
1) 2H2O → O2 + 2H2 ∆H= +572 kJ
2) N2O5 + H2O → 2HNO3 ∆H= -78 kJ
3) N2 + 3O2 + H2 → 2HNO3 ∆H= -349 kJ
Issue 5
The data in the table below was compiled for the following reaction.
A + B → C + D
At temperature T, the following initial velocity data was obtained.
|
Experience |
[A] (mol/L) |
[B] (mol/L) |
Initial speed (mol/L s) |
|
1 |
0,020 |
0,020 |
5,0 x 10-3 |
|
2 |
0,040 |
0,020 |
1,0 x 10-2 |
|
3 |
0,040 |
0,060 |
4,5 x 10-2 |
Determine the rate law equation and the rate constant at temperature T with the appropriate units.
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