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UI CHEM 001 Best Chemistry Thermochemistry Solutions Practice Exam
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Provides an introductory theory of thermochemistry and the best 20 questions with answers with varying levels of difficulty from easy to olympiad level

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  • November 23, 2022
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  • 2022/2023
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Best Chemistry Thermochemistry Solutions Practice Exam
University of Indonesia CHEM 001
20’s Thermochemistry Practice Exam Solutions


Thermochemistry

Exothermic and Endothermic Reactions

Reactant Product
HR Hp Enthalpy
Enthalpy Change: H = HP – HR
Exothermic Reaction: H = HP – HR < 0
Endothermic Reaction: H = HP – HR > 0




Thermochemistry Equation

H2(g) + ½ O2(g) H2O (l) H = -286 kJ
Especially in thermochemistry equations Coefficient = Mole

If the coefficient of a thermochemistry equation is multiplied by a certain
number, then the H is also multiplied by that number:
H2(g) + ½ O2(g) H2O (l) H = -286 kJ
2 H2(g) + O2(g) 2 H2O (l) H = -572 kJ

If the thermochemical equation is reversed, then H is given the opposite sign
H2(g) + ½ O2(g) H2O (l) H = -286 kJ
H2O (l) H2(g) + ½ O2(g) H = +286 kJ

,Molar Enthalpy

Standard Enthalpy of Formation (Hf°)(25°C, 1atm)
Hf° CO2(g) = -394 kJ/mole
C(s) + O2(g) CO2(g) H = -394 kJ/mole

Standard Enthalpy of Decomposition (Hd°)(25°C, 1atm) Hd° = - Hf°
Hd° CO2(g) = +394 kJ/mole
CO2(g) C(s) + O2(g) H = +394 kJ/mole

Standard Enthalpy of Combustion (Hc°)(25°C, 1atm) Generally exothermic
Hc° H2(g) = -286 kJ/mole
H2(g) + ½ O2(g) H2O (l) H = -286 kJ/mole
So, Hc° H2(g) = Hf° H2O(l)

Enthalpy of Neutralization (Hn°)
The enthalpy change for the reaction between an acid (H+) and a base (OH-)
forms 1 mole of water
HCN(aq) + NaOH(aq) NaCN(aq) + H2O(l) H = -12 kJ/mole

Enthalpy of Fusion (Hfus°)
H2O (s) H2O(l) H = +6 kJ/mole

Enthalpy of Solution (Hs°)
NaCl(s) Na+(aq) + Cl-(aq) H = +4 kJ/mole

, Determination of H by experiment (Calorimeter)

Q = amount of calories
Qsolution = mc T
m = the mass of the solution in the calorimeter
Qcalorimeter = C T
c = specific heat of solution in the calorimeter
Qreaction = Qsolution + Qcalorimeter C = heat capacity of the calorimeter
H = - Qreaction T = temperature change in the calorimeter
𝐻 H = reaction enthalpy change
H°=
𝑛 H°= standard enthalpy change for the reaction
n = moles of substance involved




The determination of H based on standard formation enthalpy
change data (Hf°)


aA + bB cC + dD H = ?

H° = (c. Hf°C + d. Hf°D) – (a. Hf°A + b. Hf°B)

H° = Hf° product - Hf° reactant
Hf° for free elements is zero

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