CHM201

Category: CHM201

ATTENTION:

Kindly note that you will be presented with 50 questions randomized from the NOUN question bank. Make sure to take the quiz multiple times so you can get familiar with the questions and answers, as new questions are randomized in each attempt.

Good luck!

CHM201

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1. The ___________ scale of temperature has absolute zero for its zero point

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2. The ___________ law of thermodynamics discusses entropy.

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3. ______________ is the amount of heat required to melt one gram of substance at its melting point.

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4. The pH of an aqueous solution which is 0.0020 M is _________

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5. A solution of a weak acid and its salt is known as a ________ solution

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6. The first law of thermodynamics deals with _________

A. conservation of energy

B. absolute zero temperature.

C. thermodynamic equivalence

D. entropy

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7. Only __________ substances can undergo electrolysis.

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8. A (an) ___________ system is one which neither shows exchange of heat nor mass with its surroundings

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9. Equilibrium is a state of dynamic molecular behaviour, meaning that ___________

A. the reaction eventually comes to a stop.

B. reactants turn into products and products turn into reactants at different rates.

C. products continually turn into reactants at a progressively faster rate.

D. reactants turn into products and products turn into reactants at equal rates

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10.

Every type of chemical bond contains a certain amount of energy. The total bond energy, which is essentially equivalent to the total potential energy of the system, is a quantity known
as: ____________

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11. The first law of thermodynamics deals with ____________

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12. Which of these is true of an isochoric system?

A. Takes place at constant temperature

B. Volume remains constant

C. Pressure is not constant

D. Heat is allowed into the system but not allowed out of the system

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13. The total energy of the universe is constant. This is a statement of the ___________ law of thermodynamics

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14. The temperature at which the motion of particles theoretically ceases is known as ___________ zero.

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15. The sum of all exponents of concentration terms in the rate equation is called __________

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16. The factor that affects the rate of reaction is ___________

A. Nature and concentration of the reactants

B. All of these

C. Temperature of the reactants

D. Catalyst

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17. If the rate of a reaction increases by a factor of 9 when the concentration of a reactant is tripled, then the reaction is ___________order with respect to that reactant.

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18. The term -dx/dt in a rate expression refers to the ________

A. increase in concentration of the reactants

B. Change in concentration of the reactants with time

C. instantaneous rate of the reaction

D. Average rate of the reaction

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19. The _________ scale of temperature has absolute zero for its zero point

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20. In general, the rate of a reaction can be increased by all the factors except ___________

A. Increasing the activation energy

B. Increasing the temperature

C. Using a catalyst

D. Increasing the concentration of reactants

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21. The reactions with the high value of energy of activation are _________

A. Moderate

B. Not feasible

C. Slow

D. Fast

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22. Which of the followings is not a type of system?

A. Closed

B. Isolated

C. Intensive

D. Open

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23. Which of the following statements is correct?

A. both temperature and heat are intensive properties

B. temperature is an intensive property while heat is an extensive property

C. Temperature is an extensive property while heat is an intensive property

D. both temperature and heat are extensive properties.

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24. The change in entropy for any process is not dependent upon the pathway by which the process occurs. In order words, the change in entropy for any process is a _________ function

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25. In order for a reaction to occur, the particles must __________

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26. _____________ Variables are independent of the mass of material.

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27. The entropy of a pure crystal at 0 K is _________ J/K.

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28. Which of these is not an extensive property of a system?

A. Density

B. Mass

C. Volume

D. Energy

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29. Free energy change at equilibrium is ___________

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30. Which of the following statements describes an isolated system?

A. No exchange of matter and energy with the surrounding is possible

B. exchange of both matter and energy with the surrounding is possible

C. only exchange of matter with the surrounding is possible

D. only exchange of energy with the surrounding is possible

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31. If more collisions can be made to take place in a given time, the rate of the reaction will ___________

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32. __________ Variables are dependent on the mass of the material.

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33. The higher the pH, the ___________ the acidity

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34. Rate of reaction is defined as the __________

A. Rate of change of concentration Of either reactant or product per unit time

B. None of the above

C. Rate of change of conc. of product only

D. Rate of change of conc. of reactant only

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35. The minimum additional energy, above the average internal energy, which the reacting molecules must possess so that their collision result in a reaction is known as ____________

A. Kinetic energy

B. Activation energy

C. Thermodynamic energy

D. Threshold energy

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36. A process taking place at constant pressure is termed _________

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37. A substance that is capable of acting as both an acid and as a base is ______________

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38. The ___________ law of thermodynamics discusses entropy.

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39. The conjugate base of HCl is __________

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40. A reaction catalyzed by light is called a ___________ reaction

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41. Milk sours more rapidly in summer than in winter because ____________

A. none of the above

B. in summer, the temperature Is high due to which effective collisions increase and hence the rate of reaction becomes fast

C. in summer, the energy of activation decreases and hence the of reaction becomes fast

D. in winter, number of molecules per unit volume increases and hence the rate of reaction becomes fast

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42. One mole of an ideal gas is heated at a constant pressure of 101300 $N m^{-2}$, from 273.2 K to 373 K. Calculate the work involved R = 8.314 J/mol/K).

A. 8314 J/mol

B. 8.314 J/mol

C. 831.4 J/mol

D. 83.14 J/mol

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43. Which of the following is not a state function?

A. entropy

B. work

C. enthalpy

D. free energy

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44. Rate of reaction generally ____________ with the rise of temperature.

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45. For any process, the change in entropy of the universe equals the sum of entropy changes to the system and the _________

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46. Rusting of iron Is an example of________ reaction

A. Slow

B. explosive

C. Fast

D. Moderate

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47. A process in which no heat is allowed to enter or leave a system is termed _______

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48. There are ___________ laws of thermodynamics

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49. __________ system is a system in which both energy and matter can exchange with the surroundings.

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50. 1g of ice will occupy __________ space than 1g of water (less/more)

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