CHE201 Final Term Past Papers

Che201 final term past papers:

MCQs

1. Thermodynamics is the study of heat.
2. Two systems in thermal equilibrium with each other have the same temperature.
3. Two systems that are each found to be in thermal equilibrium with a third system will be found to be in thermal equilibrium with each other.is called Zeroth law of

thermodynamics

4. The quantitative study and measurement of heat and enthalpy changes is known as thermochemistry.
5. The measurement of q or ΔH is generally known as Calorimetry
6. Example of a irreversible process is Heat transfer
7. The oxidation of gold is Nonspontaneous Processes
8. The reaction quotient Q is a measure of the relative amounts of products and reactants present in a reaction at a given time.
9. Gibbs Helmholtz demonstrate that the free energy, not heat production, was the driver of spontaneous change in isothermal chemical reactions.
10. The molarity (M) of a solution is used to represent the amount of moles of solute per liter of the solution.
11. Foams are liquids or solids with a gas dispersed into them.
12. The interactions between the solute particles and the solvent molecules is called

solvation

13. Dissolution, the solute separates into ions or molecules, and each ion or molecule is surrounded by molecules of solvent.
14. Chemical kinetics is the measurement of how quickly reactions occur.
15. The fractionating column is packed with glass beads (or something similar) to give the maximum possible surface area for vapor to condense on.
16. The continuous flow assay offers a high degree of accuracy by allowing what amounts to a large number of readings at each time point,
17. The initial rate of reaction is the rate at which the reagents are first brought together
18. Relaxation method: Many chemical reactions are complete in less than a few seconds, which makes the rate of reaction difficult to determine. In these cases, the relaxation methods can be used to determine the rate of the reaction
19. Although a balanced chemical equation for a reaction describes the quantitative relationships between the amounts of reactants present and the amounts of products that can be formed,
20. A first-order reaction is a reaction that proceeds at a rate that depends linearly on only

one reactant concentration

21. In Third Order Reaction,the minimum number of molecules necessary for the reaction to take place is three.
22. Third order reaction does not depend on Product concentration.
23. The activation energy is the threshold energy that the reactant(s) must acquire before

reaching the transition state

24. The kinetic energy of a molecule is proportional to the velocity of the molecule.
25. Once started, chain reactions continue until the reactants are exhausted
26. A mixture of hydrogen and chlorine will not react at all in the dark
27. the concentrations of the different reactants will generally fall at different rates, depending on the stoichiometry.
28. Chain reactions usually consist of many repeating elementary steps, each of which has a chain carrier.
29. Whether you use the differential rate laws or the integrated laws, you have to evaluate the order first.
30. The classical examples of such reactions are two of the fastest ones ever observed, the

dissociation of water

1. Effect of the catalyst on the energy of activation 2 (Topic 101,115)
2. Pseudo first order reaction 2 (Topic 105)
3. Define solubility 2 (Topic 77)
4. Elementary steps for the reaction mechanism 3 (Topic 126-127)
5. Properties of colloids 3 (Topic 76)
6. Mechanism of stopped flow 3 (Topic 145)

What are the limitations of thermodynamics 5 (Topic 134-135) Define the half-life of reaction, Discuss half-life of 0, 1st and 2nd order reactions 10 (Topic 109-110-111-112) Factors that affect the reaction rate 10 (Topic 100-101)

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Che201

Very easy tha.

1. effect of catalyst
2. pseudo first order reaction
3. properties of colloids
4. stopped flow method
5. elementary steps for reaction mechanism.
6. le chateliers principle
7. azeotrops
8. open, close and isolated system
9. half life reaction, zero, 1St and second order reaction.

che201

Define chemical system.

Effect of catalyst on activation energy. Limitations of thermodynamic reaction. What is half life?half life of zero first second order of reaction. Define closed isolated and open system. Colloid define. Azeotropes . Flow mechanism reaction. Le chateliers principal effect on temperature and pressure.

Che201

Gibbs free energy (2) Effect of catalyst on energy of activation (2)

Open, closed and isolated systems (3)

Limitations of thermodynamics (5) Le Chàtelier's principle with effect of concentration, temperature and pressure (5) Azeotropes (5) Define half life and also discuss half lives of zero, first and second ordered reactions (10)