Pearson Edexcel International GCSE (9–1) · CHEMISTRY · Unit
Physical Chemistry
442 practice questions
Topics covered
Practice questions
101–110 of 442
Question 101
3 marks · Easy
Answer and see the solution →Bond energies are given below:
Bond Bond energy / kJ mol^{-1} N≡N 946 H–H 436 N–H 388 Use the bond energies to answer the following about the reaction:
(a)[1 mark]Calculate the total energy needed to break all bonds in the reactants.
(b)[1 mark]Calculate the total energy released by forming all bonds in the products.
(c)[1 mark]Determine the enthalpy change (ΔH) for the reaction.
Question 102
2 marks · Easy
Answer and see the solution →The reaction below occurs: Bond energies (kJ/mol): HI: 299, H–H: 436, I–I: 151 Calculate the enthalpy change (ΔH) for the reaction.
Question 103
2 marks · Normal
Answer and see the solution →State the meaning of the term 'bond energy' and give the unit in which it is measured.
Question 104
4 marks · Normal
Answer and see the solution →The reaction between ethane and chlorine is represented by the following equation:
Use the bond energies given below for your calculations.
Bond Energies Bond Bond energy / kJ mol^{-1} C–H 413 C–C 348 C–Cl 338 Cl–Cl 243 H–Cl 432 (a)[1 mark]List all bonds that are broken and all bonds that are formed in this reaction.
(b)[1 mark]Calculate the total energy required to break the bonds in the reactants.
(c)[1 mark]Calculate the total energy released when new bonds are formed in the products.
(d)[1 mark]Calculate the enthalpy change () for the reaction. State whether the reaction is exothermic or endothermic.
Question 105
3 marks · Normal
Answer and see the solution →Calculate the enthalpy change () for the reaction:
Bond Energies (kJ/mol) Bond Bond energy / kJ mol^{-1} H–H 436 O=O 498 O–H 464 Question 106
3 marks · Normal
Answer and see the solution →Explain why the reaction between hydrogen and chlorine to form hydrogen chloride is exothermic, making reference to bond energies:
Bond energies (kJ/mol):
Bond Bond energy H–H 436 Cl–Cl 243 H–Cl 432 Question 107
4 marks · Normal
Answer and see the solution →The following data show bond energies for several bonds:
Bond Energies for Calculation Bond Bond Energy / kJ mol^{-1} C–H 413 O=O 498 C=O 743 O–H 464 (a)[1 mark]Consider the equation:
Count and list all the bonds broken in the reactants.
(b)[1 mark]Count and list all the bonds formed in the products.
(c)[1 mark]Calculate the total energy absorbed in breaking the bonds in the reactants.
(d)[1 mark]Calculate the enthalpy change () for the reaction.
Question 108
1 mark · Normal
Answer and check →Which statement is correct about bond energies and enthalpy change in chemical reactions?
- A.Bond making requires energy and is endothermic.
- B.Breaking bonds releases energy and is exothermic.
- C.Bond making releases energy and is exothermic.
- D.Breaking bonds releases energy and is endothermic.
Question 109
2 marks · Normal
Answer and see the solution →State two reasons why calculated enthalpy changes using bond energies are only estimates and not always exactly the same as values from calorimetry experiments.
Question 110
4 marks · Normal
Answer and see the solution →Consider the following reaction:
Given the following bond energies (kJ/mol):
Bond Energies Bond Bond energy C–H 413 F–F 158 C–F 485 H–F 565 (a)[1 mark]List all the bonds to be broken in the reactants.
(b)[1 mark]Calculate the total energy required to break these bonds.
(c)[1 mark]Calculate the total energy released when new bonds are formed in the products.
(d)[1 mark]Calculate the overall enthalpy change (ΔH) for the reaction.