Energetics
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This document describes procedures for determining standard enthalpy changes of neutralization, combustion, and chemical reactions. It includes typical experimental setups, tables and graphs of data, and calculations for determining the standard enthalpy change from the temperature change of a reaction using calorimetry principles. Considerations for accuracy such as insulation, heat capacity effects, and completeness of reactions are also discussed.
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INTRODUCTION
Chemical reactions are generally accompanied by some heat change. The chemical reactions which involve energy changes are referred to as thermochemical reactions. During many chemical reactions, energy is converted to heat energy and result in increase in the temperature of the surrounding. These reactions are called exothermic reactions. Some chemical changes absorb energy from the surrounding and are known as endothermic reactions.
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CH3COOH + NaOH = CH3COONa + H2O + heat
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1. The document provides instructions for an experiment to determine the heat of neutralization of hydrochloric acid (HCl) and sodium hydroxide (NaOH) through calorimetry.
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Ptotal = PN2 + PO2 + PCO2
2.50 atm = 0.90 atm + 0.60 atm + PCO2
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- The entropy of the mixture is also the sum of the individual components and obeys the second law of thermodynamics.
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Chemical process calculations involve various computations and analyses to design, optimize, and understand chemical processes. Here are some descriptions highlighting different aspects of chemical process calculations:
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These calculations involve tracking the flow rates and compositions of substances throughout a process, often using mass or mole balances.
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Reaction Kinetics:
Chemical reactions kinetics calculations focus on understanding the rates at which reactions occur and how they are influenced by various factors such as temperature, pressure, and catalysts.
These calculations help in determining the optimal reaction conditions and designing reactors for desired conversion rates.
Phase Equilibrium Calculations:
Phase equilibrium calculations deal with determining the distribution of components between different phases in a system, such as liquid-liquid or vapor-liquid equilibrium.
These calculations are essential for designing separation processes like distillation, extraction, and absorption.
Thermodynamic Calculations:
Thermodynamic calculations involve applying thermodynamic principles to predict the behavior of chemical systems.
These calculations include determining properties such as enthalpy, entropy, Gibbs free energy, and fugacity, which are crucial for process design and optimization.
Process Simulation:
Process simulation involves using computer software to model and simulate chemical processes.
These simulations allow engineers to predict process behavior under different operating conditions, optimize process parameters, and troubleshoot potential issues.
7
network error
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This document discusses colligative properties, which are physical properties of solutions that depend on the concentration of solute particles rather than the identity of the solute. It defines key colligative properties like boiling point elevation, freezing point depression, and osmotic pressure. The document also explains how these properties obey mathematical relationships like Raoult's law. Several examples are provided to demonstrate how to use these relationships and colligative property equations to calculate values like vapor pressure, boiling point, freezing point, osmotic pressure, and molar mass of a solute.
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Energetics
- 2. Standard enthalpy change of neutralisation 0 Definition 0 Dependent variable 0 Independent variable 0 Value of Hneut o 0 Basicity of acids
- 4. For each set of data Amt. of HCl Amt. of NaOH Initial temp. of HCl Initial temp.of NaOH Ave. initial temp.
- 5. Typical Table of Data Amt. HnX Amt. NaOH Max. temp. T = Tmax - Tinitial 50 10 40 20 30 30 20 40 10 50 For example, using 1 mol dm-3 acid and NaOH HnX + nNaOH NanX + nH2O Better than the word “Final”
- 6. Typical Graph – type 1 Vol. of NaOH used / cm3 10 20 30 40 50
- 7. If Basicity of acid, n = 1 Amt. HnX Amt. NaOH Max. temp. T = Tmax - Tinitial 50 10 40 20 30 30 20 40 10 50
- 8. Work out using HCl Amt. HCl Amt. NaOH Hneut o 50 10 - 60 x c x T1 0.01 40 20 - 60 x c x T2 0.02 30 30 - 60 x c x T3 0.03 20 40 - 60 x c x T2 0.02 10 50 - 60 x c x T1 0.01
- 9. Typical Graph – type 2 Vol. of NaOH used / cm3 10 20 30 40 50 Type 1 Type 2
- 10. If Basicity of acid, n = 2 Amt. HnX Amt. NaOH Max. temp. T = Tmax - Tinitial 50 10 40 20 30 30 20 40 10 50
- 11. Work out using H2SO4 Amt. H2SO4 Amt. NaOH Hneut o 50 10 - 60 x c x T1 0.01 40 20 - 60 x c x T2 0.02 30 30 - 60 x c x T3 0.03 20 40 - 60 x c x T4 0.04 10 50 - 60 x c x T2 0.02
- 12. Most informative region Vol. of NaOH used / cm3 10 20 30 40 50 Type 1 Type 2 Monobasic Dibasic
- 13. Considerations for accuracy and reliability 0 Insulation – styrofoam cup, lid 0 Stability of set-up – beaker 0 thermometer – precision 0 Consistency of stirring
- 14. Standard enthalpy change of combustion 0 Definition 0 Dependent variable 0 Independent variable
- 16. Typical Table of Data 0 Initial mass of spirit lamp Final mass of spirit lamp Initial temp Max. temp. Raw Data
- 17. Work out using C2H5OH Mass of C2H5OH T Hcombustiom o - mH2O x c x T nC2H5OH Processed Data Refer to HCI/2010 for consideration on heat absorbed by Cu can.
- 18. Considerations for accuracy and reliability 0 Heat loss to surroundings – insulation of Cu can 0 Heat loss to Cu can – consider heat capacity of Cu can 0 Incomplete combustion of alcohol
- 19. If diff alcohols are used
- 20. Standard enthalpy change of reaction 0 Definition 0 Dependent variable 0 Independent variable
- 21. Na2CO3(s) + 2HCl(aq) 2NaCl(aq) + H2O(l) + CO2(g) Suitable quantities of reactants to use: 0.010 mol Na2CO3 (1.06 g Na2CO3) 0.020 mol HCl ( 20 cm3 1 mol dm-3 HCl) Mass of empty weighing bottle = Mass of weighing bottle and Na2CO3 = Mass of emptied weighing bottle and residue = Volume of HCl used = Initial temp of HCl =
- 23. Table of data Time / min Temperature / oC 0 1 2 3.5 4 5 6 7
- 24. Typical graph Temp / oC Time / min1 2 3.5 4 5 6 7
- 25. 2 3.5 Temp / oC Time / min T At 3 min, time of addition of Na2CO3
- 26. Calculate Hreaction o Hreaction o = - MHCl x c x T nNa2CO3 Assume density of HCl = 1 g cm-3 Na2CO3(s) + 2HCl(aq) 2NaCl(aq) + H2O(l) + CO2(g)
- 27. NaHCO3(s) + HCl(aq) NaCl(aq) + CO2(g) + H2O(l) T
- 28. Calculate Hreaction o Hreaction o = + MHCl x c x T nNaHCO3 Assume density of HCl = 1 g cm-3 NaHCO3(s) + HCl(aq) NaCl(aq) + H2O(l) + CO2(g)
- 29. Think about… 0 The standard enthalpy change of: Na2CO3(s) + HCl(aq) NaHCO3(aq) + NaCl(aq)