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Chapter 5: Problem 73

Using values from Appendix \(\mathrm{C},\) calculate the standard enthalpy change for each of the following reactions: (a) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) (b) \(\mathrm{Mg}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{MgO}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) (c) \(\mathrm{N}_{2} \mathrm{O}_{4}(g)+4 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)\) (d) \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(g)\)

Short Answer

Expert verified
The standard enthalpy changes (∆H°) for the given reactions are: (a) ∆H°(reaction) = -198 kJ/mol (b) ∆H°(reaction) = -37 kJ/mol (c) ∆H°(reaction) = -1284 kJ/mol (d) ∆H°(reaction) = -291 kJ/mol

Step by step solution

01

(Reaction a) Calculate ∆H° for 2SO2(g) + O2(g) → 2SO3(g)

First, look up the standard enthalpy values for the reactants and products in Appendix C. Then apply the formula mentioned above: ∆H°(reaction) = [2 × ∆H°(SO3)] - [2 × ∆H°(SO2) + ∆H°(O2)] Substitute the values from Appendix C into the equation and solve for ∆H°(reaction).
02

(Reaction b) Calculate ∆H° for Mg(OH)2(s) → MgO(s) + H2O(l)

Look up the standard enthalpy values for the reactants and products in Appendix C. Then apply the formula: ∆H°(reaction) = [∆H°(MgO) + ∆H°(H2O)] - [∆H°(Mg(OH)2)] Substitute the values from Appendix C into the equation and solve for ∆H°(reaction).
03

(Reaction c) Calculate ∆H° for N2O4(g) + 4H2(g) → N2(g) + 4H2O(g)

Look up the standard enthalpy values for the reactants and products in Appendix C. Then apply the formula: ∆H°(reaction) = [∆H°(N2) + 4 × ∆H°(H2O)] - [∆H°(N2O4) + 4 × ∆H°(H2)] Substitute the values from Appendix C into the equation and solve for ∆H°(reaction).
04

(Reaction d) Calculate ∆H° for SiCl4(l) + 2H2O(l) → SiO2(s) + 4HCl(g)

Look up the standard enthalpy values for the reactants and products in Appendix C. Then apply the formula: ∆H°(reaction) = [∆H°(SiO2) + 4 × ∆H°(HCl)] - [∆H°(SiCl4) + 2 × ∆H°(H2O)] Substitute the values from Appendix C into the equation and solve for ∆H°(reaction).

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Most popular questions from this chapter

An aluminum can of a soft drink is placed in a freezer. Later, you find that the can is split open and its contents frozen.Work was done on the can in splitting it open. Where did the energy for this work come from?

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Using values from Appendix \(\mathrm{C},\) calculate the value of \(\Delta H^{\circ}\) for each of the following reactions: (a) \(\mathrm{CaO}(s)+2 \mathrm{HCl}(g) \longrightarrow \mathrm{CaCl}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g)\) (b) \(4 \mathrm{FeO}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) (c) \(2 \mathrm{CuO}(s)+\mathrm{NO}(g) \longrightarrow \mathrm{Cu}_{2} \mathrm{O}(s)+\mathrm{NO}_{2}(g)\) (d) \(4 \mathrm{NH}_{3}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{~N}_{2} \mathrm{H}_{4}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\)
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