June Which is a closed system? (A) burning candle (B) halogen lightbulb (C) hot water in a sink (D) ripening banana

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1 June Which is a closed system? burning candle halogen lightbulb hot water in a sink ripening banana 29. Which involves the greatest energy change? chemical reaction nuclear reaction phase change physical change 30. When the contents of a cold pack are reacted, a cooling effect is observed. How does the energy of the pack and the energy of the surroundings change to get this cooling effect? 32. Which best describes the reaction below? 33. A 10.0 g sample that is 75.0% C 8 H 18 and 25.0% C 2 H 5 OH is completely combusted. Given the fuel values below, how much energy was released? 34.2 kj 77.4 kj 387 kj 432 kj 34. The molar enthalpy of combustion for glucose, C 6 H 12 O 6 (s) (molar mass = g/mol), is kj/mol. What mass of glucose must be burned to release 2430 kj of energy? 101 g 156 g 321 g 561 g 35. How much energy is required to heat 5.0 g of aluminum from 20.0 O C to O C? 13 J 17 J 360 J 450 J

2 36. The graph below represents the heating curve of a substance that starts as a solid below its freezing point. What is the melting point of this substance? 30 C 55 C 105 C 120 C 37. Water is heated from ice at 0.0 o C to vapour at o C. When does the water experience the greatest change in potential energy? at 0.0 o C 0.0 o C to o C at o C o C to o C 38. Initially a large candle is lit at one end. A student decides to light the other end so that she is burning the candle at both ends. What has doubled in this system? amount of energy released fuel value of the candle molar enthalpy of combustion temperature of the candle 39. Given the data below, what is the H rxn for: 4 FeO(s) + O 2 (g) v 2 Fe2O3(s)? -574 kj -555 kj 555 kj 574 kj 40. A student attempting to determine the molar enthalpy of combustion for ethanol uses an alcohol burner to heat a tin can which is half full of water. In calculating the energy absorbed by the water, the result obtained was lower than the accepted value. Which had the least affect on the error? amount of soot on the can amount of water in the can heat absorbed by the can distance between the burner and can 53.(a) A butane torch can be used to determine the heat capacity of antifreeze. Butane, C4H10, has a molar heat of combustion of kj/mol. List the laboratory equipment and the data needed to determine the specific heat capacity of antifreeze solution. (b) Calculate the enthalpy change for the following reaction:

3 (c) A 1.50 g sample of granola bar is placed in a bomb calorimeter with a heat capacity of 10.2 kj/ o C. When the bar is completely burned the temperature of the calorimeter and its contents increased by 3.10 o C. What is the fuel value of the bar? (d) The reaction below shows the combustion of ethyne. C 2 H 2 (g) + 2 O 2 (g) 6 2 CO 2 (g) + H 2 O(l) (i) Use the bond energies in the table below to calculate the molar heat of reaction for ethyne. (ii) A calorimetry experiment performed by a student determined the molar heat of this reaction to be kj/mol. Give two reasons why there is a difference in the H value obtained from calorimetry and the value obtained from bond energies? June Which best defines the specific heat capacity of a substance? the energy required to raise the temperature of 1.0 g of a substance 1.0 o C the energy required to raise the temperature of 1.0 g of a substance o C the energy required to raise the temperature of 1.0 mol of a substance 1.0 o C the energy required to raise the temperature of 1.0 mol of a substance o C 30. If 23.9 g of an unknown metal requires 343 J of energy to change its temperature from 24.5 o C to 85.0 o C, what is the specific heat capacity of the metal? J/g@ o C o C 4.22 o C 868 o C 31. A substance undergoes a change that causes the temperature of its surroundings to increase but the temperature of the substance remains the same. Which best explains what happens to the substance? kinetic energy decreases melts at its freezing point potential energy decreases vaporizes at its boiling point 32. Which best indicates what happens when CH 4 (g) burns according to the reaction below? 33. For the reaction below, what is the molar heat of formation of kj kj kj kj 34. What is the symbol for the enthalpy change that occurs when a substance changes from solid to liquid, under standard conditions? H o cond H o fus H o soln H o vap

4 35. How much energy is absorbed when 10.0 g of water vaporizes at o C? 4.07 kj 22.6 kj 40.7 kj 73.3 kj 36. Which is the correct order of energy changes from greatest to least? 37. What is the fuel value of a 2.00 g sample of peanut butter that produces kj of energy? kj/g 22.6 kj/g 43.2 kj/g 90.5 kj/g 38. What is the melting point of the substance in the graph below? 30 o C 60 o C 100 o C 120 o C 39. Using the thermochemical equations given, what is the enthalpy of the reaction below? kj kj 72.9 kj kj 40. If the molar heat of formation for CH 3 OH(l)is kj/mol, what is the molar heat of formation for CO(g)? kj/mol kj/mol kj/mol kj/mol

5 53. (a) In order to determine the molar heat of combustion of candle wax, C 25 H 52 (s), water is heated in an aluminum can by a candle. The following results were recorded. If the heat produced from the candle was absorbed by the water and the aluminum can, what is the molar heat of combustion of the candle wax? (b) How many moles of methanol must burn to raise the temperature of g of aluminum by 80.0 o C? Assume all heat is absorbed by the aluminum, c Al = J/g o C, and the molar heat of combustion of methanol, CH 3 OH(l), is -239 kj/mol. (c) A 20.0 g sample of NaCl(s), at o C, is heated to o C. Given the information below, calculate the total energy required to heat the sample. (d) Given the data below, calculate the energy required to break the C-H bond. June Which piece of equipment should be used to create an isolated system? aluminum can bomb calorimeter stoppered flask test tube 30. For a given substance, which process involves the largest heat change? (g) 6 (l) (g) 6 (s) (l) 6 (g) (l) 6 (s) 31. Which compound is most stable? CS 2 (g), H o f = 117 kj/mol C 2 H 4 (g), H o f = 52.4 kj/mol C 2 H 6 (g), H o f = kj/mol CO 2 (g), H o f = -394 kj/mol

6 32. A bathtub and a teacup are both full of water at 20.0 o C. Which best illustrates the relationship between the heat capacity and the specific heat capacity of the water in each? 33. If 9.54 kj of heat is required to raise the temperature of g of a substance from 20.5 o C to 45.0 o C, what is the specific heat capacity of the substance? J/g@ o C J/g@ o C 1.04 J/g@ o C 1.73 J/g@ o C 34. Given the specific heat capacity of H 2 (g) is 14.3 J/g o C, how much energy is absorbed when 2.50 g of H 2 (g) is heated from 17.0 o C to 23.0 o C? J J J J 35. How much heat is produced when moles of H 2 (g) is consumed in the reaction below? kj kj 1586 kj 3172 kj 36. Which illustrates the first law of thermodynamics? q system = -q surroundings q system = q surroundings T system = T surroundings T system = - T surroundings 37. Which describes the reaction below? 38. Which phase change has occurred for a 5.00 g sample of H 2 O if it has absorbed 1.67 kj of heat? 39. What is true of the enthalpy change for a chemical reaction? always decreases always increases is dependent on the pathway is independent of the pathway

7 40. Given the information below, what is the molar enthalpy of combustion for ethanol? kj -358 kj 358 kj 1236 kj 53. (a) 5.50 g of NaOH(s) is dissolved in 175 ml of water in a coffee cup calorimeter. If the temperature of the water increased by 2.1 o C, calculate the molar heat of solution for NaOH(s). (b) Calculate the total energy required to heat 225 g of H2O from o C to 80.0 o C. (c ice = 2.01 J/g o C) (c) Using the data below, calculate H for (d) Using the data below, calculate the enthalpy change for the following reaction. June What is the amount of heat released when the temperature of a 5.20 g iron nail changes from 22.0 EC to 38.5 o C? (c iron = J/g o C) 22.1 J 38.1 J 50.8 J 88.9 J 30. The specific heat capacity of aluminum metal is J/g o C. What is the heat capacity of a g aluminum frying pan? J/ o C J/ o C 445 J/ o C 562 J/ o C 31. Which device best measures changes in kinetic energy? beaker calorimeter thermometer voltmeter

8 32. What happens to the water in a bomb calorimeter when an exothermic reaction occurs? 33. Which enthalpy diagram and H best represent the reaction below? 34. When 1 mol of CH 3 OH(l) decomposes 129 kj of heat is absorbed. Which thermochemical equation represents the decomposition of 2 mol of CH 3 OH(l)? 2 CH 3 OH(l) kj > 2 CO(g) + 4 H 2 (g) 2 CH 3 OH(l) kj > 2 CO(g) + 4 H 2 (g) 2 CH 3 OH(l) > 2 CO(g) + 4 H 2 (g) kj 2 CH 3 OH(l) > 2 CO(g) + 4 H 2 (g) kj 35. If 5.74 kj of energy is required to melt 50.0 g of sodium metal at its melting point, what is the molar heat of fusion for sodium metal? kj/mol 2.64 kj/mol 12.5 kj/mol 287 kj/mol

9 36. The equation below shows the enthalpy change that occurs when NH4NO3 dissolves in water. Which describes this process? 37. Which statement describes the energy changes that take place when a solid changes to a liquid at a constant temperature? 38. Which involves the greatest amount of energy? combustion condensation neutralization nuclear fission 39. Which compound is most chemically stable? 40. Using the equations below, what is the enthalpy of formation of H 2 O 2 (l)? -376 kj/mol -188 kj/mol 188 kj/mol 376 kj/mol

10 53.(a) g of water at o C is cooled to 0 o C and frozen. i) Calculate how much heat is released in this process. ii) Calculate the number of moles of ammonia that can undergo a phase change from liquid to gas, using the energy from the process above. (b) Using the data determine H for the reaction below. (c) Use the data below to calculate the fuel value of propane. June Which describes an open system? matter and heat may be stationary matter and heat may be transferred only heat can flow in and out only matter can flow in and out 30. What is the temperature change for a 15 g piece of iron that absorbs 26.5 J of heat? (c Fe = J/g@EC) 0.25 EC 0.78 EC 1.3 EC 4.0 EC 31. Which refers to the amount of energy required to raise the temperature of 1.0 g of a substance by 1.0 EC? heat capacity molar enthalpy molar heat specific heat capacity 32. How much heat is absorbed by a bomb calorimeter if it increases in temperature by 23.2 EC? (C calorimeter = 17.9 J/EC) J 1.30 J 415 J J 33. When a cold pack is crushed, NH 4 NO 3 (s) dissolves in water inside the package. The pack is then used as a cooling source for muscle injuries. Which best explains what happens? The water temperature decreases due to the endothermic process. The water temperature decreases due to the exothermic process. The water temperature increases due to the endothermic process. The water temperature increases due to the exothermic process.

11 34. What change is occurring if the temperature of a substance remains constant as energy is added to it? gas to liquid gas to solid liquid to gas liquid to solid 35. At its boiling point, what mass of methanol, CH 3 OH (32.05 g/mol), is vaporized by 875 kj of heat energy? ( H vap (CH 3 OH) = 35.2 kj/mol) g 1.29 g 24.9 g 797 g 36. Which enthalpy notation represents the energy needed to melt iron? H comb H fusion H solid H vap 37. How many moles of chlorine is required to release 55.8 kj of heat? H 2 + Cl 2 2 HCl H =!335 kj moles moles 3.00 moles 6.00 moles 38. What is true for changes in the kinetic and potential energy for section B-C on the graph below? Kinetic Energy Potential Energy constant decreases constant increases decreases constant increases constant 39. Given the thermochemical equations below, what is the heat of reaction for the formation of nitrogen dioxide? NO(g) + ½ O 2 (g) NO 2 (g) ½ N 2 (g) + ½ O 2 (g) NO(g) HE = 91.3 kj ½ N 2 (g) + O 2 (g) NO 2 (g) HE = 33.2 kj!124.5 kj!58.1 kj kj kj

12 40. Using the reactions and data given, what is the bond energy for Cl-Cl? H 2 (g) + Cl 2 (g) 2 HCl(g) kj Bond Bond Energy (kj/mol) H-H 436 H-Cl kj/mol 336 kj/mol 520 kj/mol 613 kj/mol 53.(a) A g chocolate bar (C 7 H 8 N 4 O 2 ) is burned in a bomb calorimeter that has a heat capacity of 6.50 kj/ec. Calculate the molar heat of combustion of the chocolate bar if the temperature of the calorimeter and its contents increases from EC to EC. (b) (c) (d) A mixture of g of an unreactive metal and g of water has a temperature of 25.0 EC. The mixture is heated to a final temperature of 70.0 EC. Calculate the specific heat capacity of the metal if the mixture absorbs 49.7 kj of heat. A 2.50 g sample of water is cooled from 95.0 EC to 0.00 EC and is completely frozen. i) Draw the cooling curve for this process. ii) Calculate the energy released by the water sample. Calculate the enthalpy change for the reaction below. 3 NO 2 (g) + H 2 O(l) 2 HNO 3 (l) + NO(g) Substance H f E (kj/mol) HNO 3 (l)!174.1 H 2 O(l)!285.8 NO(g) 91.3 NO 2 (g) 33.2

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