Buy Exothermic and Endothermic Reactions

Buy Exothermic and Endothermic Reactions
Buy Exothermic and Endothermic Reactions
Quick questions
1 The reaction between zinc and copper sulfate solution causes the
temperature of the solution to rise. Is the reaction exothermic or
endothermic?
2 Give one example of an application of an endothermic reaction.
3 Give one variable that would affect the temperature change when
hydrochloric acid reacts with magnesium metal.
4 Define the term ‘activation energy’.
5 State which quantity is greater for an endothermic reaction: the
amount of energy absorbed during bond breaking, or the amount
of energy released during bond making.
Exam-style questions
6 When ammonium nitrate, NH4NO3, is dissolved in water the
temperature of the solution formed decreases.
NH4NO3(s) water → NH4NO3(aq)
A student investigated how the mass of ammonium nitrate
dissolved affected the temperature change of the solution.
6–1 Write down whether the dissolving of ammonium nitrate is
exothermic or endothermic. Explain your answer. [2]
6–2 Draw a fully labelled reaction profile for the dissolving of
ammonium nitrate to form a solution. [3]
6–3 Describe a method the student could use to investigate how
the mass of ammonium nitrate dissolved affects the change in
temperature of the water. Your method should give valid results. [6]
Total: 11
p231–2 5.5.1.1
p232 5.5.1.1
p233 5.5.1.2
p235–7 5.5.1.3 MS1a
p233 5.5.1.2
p234 5.5.1.1 RP4
AT1,3,
5,6
p234 5.5.1.1 RP4
AT1,3,
5,6
p232–3 5.5.1.1
 
Buy Exothermic and Endothermic Reactions
Energy changes topic review
95
7 Hydrogen peroxide, H2O2, is a very useful compound. It is very
reactive due to the single covalent bond between the two oxygen
atoms. Hydrogen peroxide decomposes to form water and oxygen.
Figure 1 shows the displayed formulae for the decomposition of
hydrogen peroxide.
H
O
H H
O H
2 O 2 O O
Figure 1
Table 1 shows the bond energies and the overall energy change
for the decomposition of hydrogen peroxide. Calculate the bond
energy X for the O–O bond in hydrogen peroxide. Use Figure 1
and Table 1. [4]
H-O O-O O=O Overall energy change
Energy in kJ/mol 463 X 496 –208
Table 1
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