1. What is meant by the term exothermic?

Question 1 of 16

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

Question 2 of 16

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

Question 3 of 16

4. What is meant by the term endothermic?

Question 4 of 16

5. Are neutralisation reactions exothermic or endothermic?

Question 5 of 16

6. Is breaking bonds exothermic or endothermic?

Question 6 of 16

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

Question 7 of 16

8. What does this diagram represent?

Question 8 of 16

9. What does this diagram represent?

Question 9 of 16

10. In a combustion calorimetry experiment, 0.78g of ethanol (C₂H₅OH) produced 12,540 J of heat energy. Calculate the molar enthalpy 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. In an endothermic reaction, which is greater: the energy taken in when breaking bonds or the energy released when bonds are made?

Question 12 of 16

13. State the units of molar enthalpy change.

Question 13 of 16

14. Are displacement reactions exothermic or endothermic?

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. 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 16 of 16


 

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