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 does this diagram represent?

Question 2 of 16

3. Explain, in terms of making and breaking bonds, why a reaction could be endothermic

Question 3 of 16

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

Question 4 of 16

5. What is meant by the term endothermic?

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. Is breaking bonds exothermic or endothermic?

Question 8 of 16

9. What is meant by the term exothermic?

Question 9 of 16

10. What does this diagram represent?

Question 10 of 16

11. Are combustion reactions exothermic or endothermic?

Question 11 of 16

12. Are displacement reactions exothermic or endothermic?

Question 12 of 16

13. 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 13 of 16

14. 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 14 of 16

15. 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 15 of 16

16. 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 16 of 16


 

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