1. In a combustion calorimetry experiment, 0.78g of ethanol (C₂H₅OH) produced 12,540 J of heat energy. Calculate the molar enthalpy change.

Question 1 of 16

2. What is meant by the term endothermic?

Question 2 of 16

3. In a chemical reaction, 250 kJ/mol is taken to break all the bonds and 280 kJ/mol is released when new bonds are formed. What is the overall molar enthalpy of the reaction?

Question 3 of 16

4. Explain, in terms of making and breaking bonds, why a reaction could be exothermic

Question 4 of 16

5. What does the symbol ΔH mean

Question 5 of 16

6. State the units of molar enthalpy change.

Question 6 of 16

7. Explain why experimental values of enthalpy change differ from theoretical values

Question 7 of 16

8. In a chemical reaction, the overall molar enthalpy is +87 kJ/mol. Is this reaction exothermic or endothermic?

Question 8 of 16

9. Are combustion reactions exothermic or endothermic?

Question 9 of 16

10. Use Q=mcΔT and c=4.18J/°C/g. A spatula of sodium fluoride is put into a boiling tube with 25cm³ of water. The temperature drops from 22.0°C to 18.6°C. What is the total heat energy change?

Question 10 of 16

11. In a calorimetry experiment to investigate the heat energy released by the combustion of ethanol, why should the water in the calorimeter be stirred?

Question 11 of 16

12. What does this diagram represent?

Question 12 of 16

13. When a solid dissolves, is this process exothermic or endothermic?

Question 13 of 16

14. What is meant by the term exothermic?

Question 14 of 16

15. Use Q=mcΔT and c=4.18J/°C/g. A strip of magnesium is added to a beaker with 200cm³ of copper (II) sulfate. The temperature starts at 21.7°C and rises to a maximum of 23.1°C. What is the total heat energy change?

Question 15 of 16

16. In an exothermic reaction, which is greater: the energy taken in when breaking bonds or the energy released when bonds are made?

Question 16 of 16


 

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