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. __________ system is a system in which both energy and matter can exchange with the surroundings.
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2. A process taking place at constant pressure is termed _________
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3. The total energy of the universe is constant. This is a statement of the ___________ law of thermodynamics
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4. The entropy of a pure crystal at 0 K is _________ J/K.
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5. The conjugate base of HCl is __________
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6. Only __________ substances can undergo electrolysis.
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7. 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).
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8. 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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9. 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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10. The ___________ scale of temperature has absolute zero for its zero point
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11. 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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12. A reaction catalyzed by light is called a ___________ reaction
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13. There are ___________ laws of thermodynamics
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14. The first law of thermodynamics deals with _________
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15. A (an) ___________ system is one which neither shows exchange of heat nor mass with its surroundings
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16. The rate at which a substance takes part in a chemical reaction depends upon its ____________
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17. The temperature at which the motion of particles theoretically ceases is known as ___________ zero.
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18. The ___________ law of thermodynamics discusses entropy.
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19. If more collisions can be made to take place in a given time, the rate of the reaction will ___________
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20. The first law of thermodynamics deals with ____________
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21. The reactions with the high value of energy of activation are _________
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22. 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 ____________
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23. The factor that affects the rate of reaction is ___________
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24. The higher the pH, the ___________ the acidity
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25. Which of the following expressions is associated with the law of conservation of energy?
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26. __________ Variables are dependent on the mass of the material.
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27. A process in which no heat is allowed to enter or leave a system is termed _______
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28. Which of the following statements is correct?
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29. Rusting of iron Is an example of________ reaction
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30. Rate of reaction is defined as the __________
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31. _____________ Variables are independent of the mass of material.
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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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33. 1g of ice will occupy __________ space than 1g of water (less/more)
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34. A substance that is capable of acting as both an acid and as a base is ______________
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35. A solution of a weak acid and its salt is known as a ________ solution
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36. The _________ scale of temperature has absolute zero for its zero point
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37. Equilibrium is a state of dynamic molecular behaviour, meaning that ___________
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38. Which of the followings is not a type of system?
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39. In order for a reaction to occur, the particles must __________
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40. In general, the rate of a reaction can be increased by all the factors except ___________
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41. In a reaction in which the rate of the reverse reaction is equal to the rate of the forward reaction, a state of __________ is attained.
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42. The term -dx/dt in a rate expression refers to the ________
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43. ______________ is the amount of heat required to melt one gram of substance at its melting point.
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44. The pH of an aqueous solution which is 0.0020 M is _________
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45. Which of these is not an extensive property of a system?
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46. 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 _____________
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47. Which of the following is not a state function?
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48. Which of the following statements describes an isolated system?
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49. The sum of all exponents of concentration terms in the rate equation is called __________
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50. Milk sours more rapidly in summer than in winter because ____________
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