Use the values of ΔHf^∘ in Appendix 4 to calculate ΔH^∘ for the following reactions. (See Exerci

Name: Problem 78, Chapter 6: Chemistry
Uploaded: 2020-05-09T22:37:18-08:00
Duration: 1 min 49 s
Channel: Jamie Huang
Description: Use the values of ΔHf^∘ in Appendix 4 to calculate ΔH^∘ for the following reactions. (See Exercise 77.) a. b. SiCl4(l)+2 H2 O(l) ⟶SiO2(s)+4 HCl(a q) c. MgO(s)+H2 O(l) ⟶Mg(OH)2(s)

step 1 So let's look at the first one. So the first one is an image. The first molecule is a hydrocarbo

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Use the values of $\Delta H_{\mathrm{f}}^{\circ}$ in Appendix 4 to calculate $\Delta H^{\circ}$ for the following reactions. (See Exercise 77.) a. b. $\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(a q)$ c. $\mathrm{MgO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)$

   Use the values of $\Delta H_{\mathrm{f}}^{\circ}$ in Appendix 4 to calculate $\Delta H^{\circ}$ for the following reactions. (See Exercise 77.)
a.
b. $\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(a q)$
c. $\mathrm{MgO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)$

Chemistry

Steven S. Zumdahl,… 8th Edition

Chapter 6, Problem 78

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Solved by Expert Jamie Huang

05/09/2020

Step 1

The problem statement does not provide a reaction for part a. b. To calculate the enthalpy change for the reaction, we can use the formula: ΔH° = Σ ΔHf°(products) - Σ ΔHf°(reactants) For the given reaction: SiCl4(l) + 2 H2O(l) → SiO2(s) + 4 HCl(aq) We can Show more…

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Use the values of $\Delta H_{\mathrm{f}}^{\circ}$ in Appendix 4 to calculate $\Delta H^{\circ}$ for the following reactions. (See Exercise 77.) a. b. $\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{SiO}_{2}(s)+4 \mathrm{HCl}(a q)$ c. $\mathrm{MgO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Mg}(\mathrm{OH})_{2}(s)$

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Key Concepts

Standard Enthalpy of Formation

This is the change in enthalpy when one mole of a compound is formed from its elements in their standard states under standard conditions. It provides a reference to calculate the energy changes in chemical reactions, and values for various substances are tabulated in standard reference materials.

Hess's Law

Hess's Law states that the overall enthalpy change for a chemical reaction is the same regardless of the path taken, allowing one to calculate reaction enthalpies by summing the standard enthalpies of formation of the products and subtracting those of the reactants.

Reaction Enthalpy Calculation

This involves using the concept of standard enthalpies of formation along with Hess's Law. The reaction enthalpy is determined by multiplying the standard enthalpy of formation of each species by its corresponding stoichiometric coefficient in the balanced equation and then subtracting the total for the reactants from that for the products.

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