ENERGY CHANGES IN CHEMICAL REACTIONS
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1 ENERGY CHANGES IN CHEMICAL REACTIONS 1. Use the information below to answer the questions that follow: Equation: Enthalpy of formation. (i) H 2(g) + ½ O 2(g) H 2 O (l) H 1 = -286kJmol -1 (ii) C (s) + O 2(g) CO 2(g) H 2 = -394kJmol -1 (iii) 2C (s) + 3H 2(g) + ½ O 2(g) C 2 H 5 OH (l) H 3 = -277kJmol -1 Calculate the molar enthalpy of combustion of ethanol. Given that: C 2 H 5 OH (l) + 3O 2(g) 2CO 2(g) + 3H 2 O (l) (3mks) 2. Study the information in the table below and answer the questions that follow Bond Bond energy (KJmol -1 ) C H 414 Cl Cl 244 C Cl 326 H - Cl 431 Calculate the enthalpy change of the reaction CH 4(g) + 2Cl 2(g) CH 2 Cl 2(g) + 2HCl (g) (3mks) 3. When 25 cm 3 of 0.5MHCl is added to 25 cm 3 of 0.5 M NaOH the temperature of the solution rose from 25 0 C to 26 0 C. Given that the density of the solution is 1g cm -3 and its specifc heat capacity is 4.2 jg -1 k -1,
2 a. Determine the amount of heat evolved that caused the temperature rise. (1mark) b. Work out the molar enthalpy of neutralization for this reaction. (2marks) 4. Study the following equilibrium equation. 2A 2(g) + B 2(g) 2A 2 B (g) H = -197KJmol -1 a) Suggest two ways of increasing the yield of A 2 B. (2mks) b) Draw the energy level diagram for the forward reaction. (1mk) 5. Use the data below to calculate the enthalpy of formation of propane. (3mks) C (g) + O 2(g) CO 2(g) H=-393.5KJmol -1 H 2(g) + ½ O 2(g) H 2 O (l) H = KJmol -1 C 3 H 8(g) + SO 2 3CO 2(g) + 4H 2 O 2(l) H= KJmol -1
3 6. Study bond energies shown below and answer the questions that follow. Bond Bond Energy KJmol -1 C C 348 C H 412 Cl Cl 242 C Cl 338 H Cl 431 a) Calculate the enthalpy change ( H) for the reaction given below. C 3 H 8(g) + Cl 2(g) C 3 H 7 Cl + HCl (2mks) b) State the condition necessary for the above reaction to occur. (1mk) g of ethanol (C 2 H 5 OH) were completely burnt in air. The heat evolved caused the temperature of 400cm 3 of water to rise from 22 0 C to 87 0 C. Calculate the molar heat of combustion of ethanol (H=1, C=12, O=16, specifc heat capacity of water = 4.2 kjkg -1 k -1 ; Density of water = 1gcm -3 )
4 (3mks) 8. (a) Consider the following reaction: A2( g ) B2 ( g ) 2AB g DH 75KJ Sketch an energy level diagram showing the relative activation energies for the catalysed and uncatalysed reactions using the axes below. ( 2 marks) Energy (KJ) Reaction path (b) Given H f H f Al2O Cr O 1134KJ mol 2 3 KJ mol 1 Calculate the heat of reaction for 2 3 Al s Cr2O Al O 2Cr s 3 s 2 (2marks) a) The following data was obtained during an experiment Mass of ethanol burnt = 0.2g Mass of water in the calorimeter = 200g Specifc heat capacity of water = 4.2 j g -1 k -1 Initial temperature of water = C
5 Final temperature of water = C (i) How was the mass of ethanol that burnt determined? (1mark) (ii) How much heat was required to raise the temperature of water from C to C? (2marks) (iii) Two assumptions were made in calculating the enthalpy of combustion for ethanol. State them. (1mark) (iv) Determine the molar enthalpy of combustion of ethanol (2marks) (C= 12, H=1, O= 16) (v) Write a thermochemical equation for the combustion of ethanol given the accurate value for enthalpy of combustion is Kj mol -1. (1mark)
6 9. Iron fllings were thoroughly mixed with sulphur then placed in two test tubes as shown below. Both test tubes were cooled to room temperature then 3cm 3 of 2M Hydrochloric acid was added. a) What is the general name given to the substance in. (2mks) (i) Test tube A (ii) Test tube B b) Identify the gas produced when 2M Hydrochloric acid was added to test tube A. Explain your answer. (2mks) c) Write an equation for the reaction that takes place when 2M Hydrochloric acid is added to test tube B. (1mk)
7 d) In another experiment excess iron powder was added to 25.0cm 3 of 0.2M copper II sulphate solution in a plastic cup wrapped in tissue paper. The temperature of this solution rose from C to C. (i) What was the main reason for using a plastic cup wrapped in tissue paper? (1mk) (ii) Give reason for using excess iron powder. (1mk) (iii) State two other observations made in the above experiment. (2mks) (iv) Calculate the molar enthalpy of displacement of copper II ions by iron powder. (3mks) (Density of solution =1.0gcm -3 heat capacity of soln 4.2J/g/k.) v) Write a Thermo chemical equation for the reaction that took place. (1mk)
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Chapter 11. Thermochemistry. 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages
Chapter 11 Thermochemistry 1. Let s begin by previewing the chapter (Page 292). 2. We will partner read Pages 293-94 The Flow of energy - heat Thermochemistry concerned with the heat changes that occur
Chemistry Slide 1 of 33
Chemistry 17.2 1 of 33 17.2 Measuring and Expressing Enthalpy Changes A burning match releases heat to its surroundings in all directions. How much heat does this exothermic reaction release? You will