In this experiment you will determine the enthalpy change, $$$\Delta H$$$, for the reaction between aqueous copper(II) sulfate and magnesium. $$\[ \mathrm{CuSO}_{4}(\mathrm{aq})+\mathrm{Mg}(\mathrm{s}) \rightarrow \mathrm{Cu}(\mathrm{s})+\mathrm{MgSO}_{4}(\mathrm{aq}) \]$$ FA 3 is $$$1.0 \mathrm{~mol} \mathrm{dm}^{-3}$$$ copper(II) sulfate, $$$\mathrm{CuSO}_{4}$$$. FA 4 is magnesium powder, Mg. Calculations (i) Calculate the heat energy produced in the reaction. heat energy produced $$$=$$$ .......................... $$$J$$$ (ii) Determine which reactant, FA 3 or FA 4, is in excess for the reaction. Show your working. (iii) Calculate the enthalpy change, $$$\Delta H$$$, in $$$\mathrm{kJ} \mathrm{mol}^{-1}$$$, for the reaction. $$\[ \Delta H=\underset{\text { (sign) }}{\ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots \ldots}{ }_{\text {(value) }} \mathrm{kJ} \mathrm{mol}^{-1} \]$$

Chemistry

IGCSE&ALevel

CAIE

Exam No：9701_m24_qp_33 Year：2024 Question No：(b)

Answer:

Knowledge points:

5.1.1 understand that chemical reactions are accompanied by enthalpy changes and these changes can be exothermic (ΔH is negative) or endothermic (ΔH is positive)

5.1.2 construct and interpret a reaction pathway diagram, in terms of the enthalpy change of the reaction and of the activation energy

5.1.3.1 standard conditions (this syllabus assumes that these are 298 K and 101 kPa) shown by

5.1.3.2 enthalpy change with particular reference to: reaction, , combustion, , neutralisation,

5.1.4 understand that energy transfers occur during chemical reactions because of the breaking and making of chemical bonds

5.1.5 use bond energies (ΔH positive, i.e. bond breaking) to calculate enthalpy change of reaction

5.1.6 understand that some bond energies are exact and some bond energies are averages

5.1.7 calculate enthalpy changes from appropriate experimental results, including the use of the relationships q = mcΔT and ΔH = –mcΔT/n

Answer:

Knowledge points:

Solution:

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