Question

Calculate $\Delta H^{\circ}$ for the process $\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s)$ from the following information: $\mathrm{Zn}(s)+\mathrm{S}(s) \longrightarrow \mathrm{ZnS}(s) \quad \Delta H^{\circ}=-206.0 \mathrm{kJ}$ $\mathrm{ZnS}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) \quad \Delta H^{\circ}=-776.8 \mathrm{kJ}$

Name: Problem 64, Chapter 5: Chemistry
Uploaded: 2021-06-15T01:15:37-08:00
Duration: 2 min 16 s
Channel: Tianyu Li
Description: Calculate ΔH^∘ for the process Zn(s)+S(s)+2 O2(g) ⟶ZnSO4(s) from the following information: Zn(s)+S(s) ⟶ZnS(s) ΔH^∘=-206.0 kJ ZnS(s)+2 O2(g) ⟶ZnSO4(s) ΔH^∘=-776.8 kJ

   Calculate $\Delta H^{\circ}$ for the process $\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s)$
from the following information:
$\mathrm{Zn}(s)+\mathrm{S}(s) \longrightarrow \mathrm{ZnS}(s) \quad \Delta H^{\circ}=-206.0 \mathrm{kJ}$
$\mathrm{ZnS}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) \quad \Delta H^{\circ}=-776.8 \mathrm{kJ}$

Chemistry

Paul Flowers, Klaus… 2nd Edition

Chapter 5, Problem 64

Instant Answer

Solved by Expert Tianyu Li

06/15/2021

Step 1

By observation, we can see that the new equation is just the sum of the given reactions. Mathematically, we can represent this as: \[\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) = \mathrm{Zn}(s)+\mathrm{S}(s) Show more…

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Calculate $\Delta H^{\circ}$ for the process $\mathrm{Zn}(s)+\mathrm{S}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s)$ from the following information: $\mathrm{Zn}(s)+\mathrm{S}(s) \longrightarrow \mathrm{ZnS}(s) \quad \Delta H^{\circ}=-206.0 \mathrm{kJ}$ $\mathrm{ZnS}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{ZnSO}_{4}(s) \quad \Delta H^{\circ}=-776.8 \mathrm{kJ}$

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Key Concepts

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the same regardless of the pathway taken, because enthalpy is a state function. This allows the use of known enthalpy changes of intermediate reactions to determine the enthalpy change for an overall reaction by simply adding them together.

Standard Enthalpy Change

Standard enthalpy change refers to the change in enthalpy when a reaction occurs under standard conditions. It is a measure of the heat absorbed or released and is typically used in thermodynamic calculations to assess energy changes in chemical processes.

Additivity of Reaction Enthalpies

Because enthalpy is a state function, the net enthalpy change of a complex reaction can be obtained by summing the enthalpy changes of its individual steps. This additivity property is fundamental in calculating the overall energy change for reactions where the process can be broken down into multiple stages.

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