- •1.2 THEORETICAL INTRODUCTION
- •1.3. WORK SEQUENCE
- •1.4 APPENDIX
- •1.5 TEST QUESTIONS
- •1.6 REFERENCES
- •2 LABORATORY PRACTICUM: EQUILIBRIUM OF HOMOGENEOUS CHEMICAL SYSTEMS
- •2.1 THEORETICAL INTRODUCTION
- •3.1. THEORETICAL INTRODUCTION
- •2.2. TEST QUESTIONS
- •2.3. REFERENCES
- •Limited Mutual Solubility of Liquids
- •Distribution of the Third Component between Two Immiscible Liquids
- •The used research method is titration.
- •Experiment Procedure
- •The used research method is titration.
- •The used research method is titration.
- •Reagents and materials: a 0.05 M (0.1 N) iodine solution in carbon tetrachloride, a 0.001 M sodium thiosulphate (Na2S2O3) solution, and a 1% freshly prepared aqueous solution of starch.
- •3.2. TEST QUESTIONS
- •3.3. TASKS FOR SELF-STUDY
- •=const,
- •Solution. Let us calculate the K values by the equation,
- •Taking a logarithm of both parts of the expression, one finds that
- •b) The following equation should be used for the case of five consecutive extractions:
- •Problems
- •3.4. REFERENCES
- •4.1. THEORETICAL INTRODUCTION
- •4.2. TEST QUESTIONS
- •LABORATORY EXERCISE 10.
- •4.3. APPENDIX
- •4.4. TEST QUESTIONS
- •4.5 REFERENCES
- •1. Explain the term "molecularity of a chemical reaction". Can the molecularity be greater or smaller than the reaction order?
- •4. Upon studying the kinetics of a chemical reaction, the kinetic curves with different concentrations of reagents have been obtained. Which of the methods of determination of the reaction order is most effective in this case?
- •w = k[HCrO4–][3HSO3–]2[H+].
- •Why is the rate of this reaction not proportional to the number of ions of each sort in accordance with the stoichiometric coefficients in the chemical equation?
- •5.2. KINETICS OF COMPLEX CHEMICAL REACTIONS
- •Task 3
- •5.3. REFERENCES
- •6. INDIVIDUAL ASSIGNMENTS. ELECTROLYTE SOLUTIONS
ddτx = k1(a − x)(b − x) −k2 (c + x) .
To which type of reactions does this reaction belong? Give its schematic representation.
6. The conversion of NH4CNS to (NH2)2CS is a reversible monomolecular reaction. Calculate the rate constants of the direct and reverse reactions at 450°C, using the following experimental data:
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τ, min |
0 |
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5 |
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12 |
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19 |
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28 |
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38 |
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48 |
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∞ |
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% of |
2 |
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3.8 |
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6.2 |
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7.1 |
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8.2 |
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10.4 |
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12.3 |
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4.2 |
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NH4CNS |
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5.3. REFERENCES |
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1. |
A.G. |
Stromberg |
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and D.P. |
Semchenko, |
Fizicheskaya |
khimiya |
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(Physical Chemistry), М.: Vysshaya shkola, 2003, 527 p. [In Russian] |
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2. |
Kratkii |
kurs fizicheskoi |
khimii |
(Brief |
Course |
of |
Physical |
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Chemistry), Textbook for institutions of higher education (Ed.: S.N. Kondratiev), М.: Vysshaya shkola, 1978, 312 p. [In Russian]
3. A.G. Golikov, Rukovodstvo po fizicheskoi khimii (Instruction Manual on Physical Chemistry), М.: Vysshaya shkola, 1988, 383 p.
4. N.M. Emmanuel and D.G. Knorre, Kurs khimicheskoi kinetiki (Course of Chemical Kinetics), Textbook for institutions of higher education, М.: Vysshaya shkola, 1984, 463 p. [In Russian]
5. G.M. Pagenkov and V.P. Lebedev, Khimicheskaya kinetika i kataliz (Chemical Kinetics and Catalysis), Textbook for institutions of higher education, М.: Khimiya, 1985, 590 p. [In Russian]
6. I.V. Kudryashov and G.S. Karetnikov, Sbornik primerov i zadach po fizicheskoi khimii (Workbook of Exercises and Problems on Physical Chemistry), М.: Vysshaya shkola, 1991, 527 p. [In Russian]
7. Kratkii spravochnik fiziko-khimicheskikh velichin (Short Handbook of Physicochemical Values (Eds.: A.A. Ravdel and A.M. ponomareva), Leningrad: Khimiya, 1983, 232 p. [In Russian]
8. Fizicheskaya khimiya v voprosakh i otvetakh (Physical Chemistry in Questions and Answers) (Eds.: K.V. Topchieva and N.V. Fedorovich), M.: Moscow State University, 1981, 24 p. [In Russian]
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