Enthalpy changes practice qs
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1 Enthalpy changes practice qs Q1. The combustion of hydrocarbons is an important source of energy. Define the term standard enthalpy of combustion. (i) Write an equation for the complete combustion of ethane, C 2H 6. (ii) Use the standard enthalpies of formation given below to calculate the standard enthalpy of combustion of ethane. Formula and state of compound C 2H 6(g) CO 2(g) H 2O(l) Standard enthalpy of formation (at 298 K)/kJ mol A container and its contents of total heat capacity 120 J K 1 were heated using a methane burner. Calculate the maximum theoretical temperature rise when 0.10 g of methane was completely burned. The standard enthalpy of combustion of methane is 890 kj mol 1. (Total 11 marks) Page 1
2 Q2. Define the term standard enthalpy of formation. State Hess s Law and use it, together with the data given in the table below, to calculate the standard enthalpy change for the following reaction. MgO(s) + 2HCl(g) MgCl2(s) + H2O(l) MgO HCl(g) MgCl 2 H 2O ΔH f /kj mol In an experiment, an excess of solid magnesium oxide was added to 50 cm 3 of 3.0 mol dm 3 hydrochloric acid. The initial temperature of the solution was 21 C. After reaction, the temperature had risen to 53 C. (The specific heat capacity of water is 4.2 J K 1 g 1 ) Use this information to calculate the enthalpy change for the reaction of one mole of magnesium oxide with hydrochloric acid. For your calculation you should assume that all the heat from the reaction is used to raise the temperature of 50 g of water. (8) (Total 15 marks) Page 2
3 Q3.A 50.0 cm 3 sample of a mol dm 3 solution of silver nitrate was placed in a polystyrene beaker. An excess of powdered zinc was added to this solution and the mixture stirred. Zinc nitrate, Zn(NO 3) 2, and silver were formed and a rise in temperature of 3.20 C was recorded. Write an equation for the reaction between silver nitrate and zinc. Calculate the number of moles of silver nitrate used in the experiment. Calculate the heat energy evolved by the reaction in this experiment assuming that all the energy evolved is used to heat only the 50.0 g of water in the mixture. (Specific heat capacity of water is 4.18 J g 1 K 1 ) (d) Calculate the heat energy change for the reaction per mole of zinc reacted. (e) Explain why the experimental value for the heat energy evolved in this experiment is less than the correct value. (Total 8 marks) Q4. Hess s Law is used to calculate the enthalpy change in reactions for which it is difficult to determine a value experimentally. State the meaning of the term enthalpy change. State Hess s Law. (1 Page 3
4 Consider the following table of data and the scheme of reactions. Reaction Enthalpy change / kj mol 1 HCl(g) H + (aq) + Cl (aq) 75 H(g) + Cl(g) HCl(g) 432 H(g) + Cl(g) H + (g) + Cl (g) +963 Use the data in the table, the scheme of reactions and Hess s Law to calculate a value for Hr (Total 5 marks) Q5. ο Define the term standard enthalpy of formation, Hf Use the data in the table to calculate the standard enthalpy of formation of liquid methylbenzene, C7H8 Substance C(s) H2(g) C7H8(l) Standard enthalpy of combustion, Hc ο /kj mol C(s) + 4H 2(g) C 7H 8(l) Page 4
5 An experiment was carried out to determine a value for the enthalpy of combustion of liquid methylbenzene using the apparatus shown in the diagram. Burning 2.5 g of methylbenzene caused the temperature of 250 g of water to rise by 60 C. Use this information to calculate a value for the enthalpy of combustion of methylbenzene, C7H8 (The specific heat capacity of water is 4.18 J K 1 g 1. Ignore the heat capacity of the container.) (d) A 25.0 cm 3 sample of 2.00 mol dm 3 hydrochloric acid was mixed with 50.0 cm 3 of a 1.00 mol dm 3 solution of sodium hydroxide. Both solutions were initially at 18.0 C. After mixing, the temperature of the final solution was 26.5 C. Use this information to calculate a value for the standard enthalpy change for the following reaction. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) In your calculation, assume that the density of the final solution is 1.00 g cm 3 and that its specific heat capacity is the same as that of water. (Ignore the heat capacity of the container.) (e) Give one reason why your answer to part (d) has a much smaller experimental error than your answer to part. Page 5 (Total 15 marks)
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