Calculate the enthalpy change for the reaction P4 O6(s)+2 O2(g) ⟶P4 O10(s) given the following e

Name: Problem 63, Chapter 5: Chemistry The Central Science
Uploaded: 2021-01-18T16:47:37-08:00
Duration: 1 min 39 s
Channel: Ronald Prasad
Description: Calculate the enthalpy change for the reaction P4 O6(s)+2 O2(g) ⟶P4 O10(s) given the following enthalpies of reaction: P4(s)+3 O2(g) ⟶P4O6(s) Δ H=-1640.1 kJ P4(s)+5 O2(g) ⟶P4O10(s) Δ H=-2940.1 kJ

step 1 Let's calculate the end to be the following reaction. So we have P406 solid to P4 solid and 302

Question

Calculate the enthalpy change for the reaction $$\mathrm{P}_{4} \mathrm{O}_{6}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)$$ given the following enthalpies of reaction: $$\begin{array}{ll}{\mathrm{P}_{4}(s)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{6}(s)} & {\Delta H=-1640.1 \mathrm{kJ}} \\ {\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)} & {\Delta H=-2940.1 \mathrm{kJ}}\end{array}$$

   Calculate the enthalpy change for the reaction
$$\mathrm{P}_{4} \mathrm{O}_{6}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)$$ given the following enthalpies of reaction:
$$\begin{array}{ll}{\mathrm{P}_{4}(s)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{6}(s)} & {\Delta H=-1640.1 \mathrm{kJ}} \\ {\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)} & {\Delta H=-2940.1 \mathrm{kJ}}\end{array}$$

Chemistry The Central Science

Theodore L. Brown 14th Edition

Chapter 5, Problem 63

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Solved by Expert Ronald Prasad

01/18/2021

Step 1

1 \mathrm{kJ} \\ \mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) &\longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s) &\Delta H_2=-2940.1 \mathrm{kJ} \end{align*} Show more…

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Calculate the enthalpy change for the reaction $$\mathrm{P}_{4} \mathrm{O}_{6}(s)+2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)$$ given the following enthalpies of reaction: $$\begin{array}{ll}{\mathrm{P}_{4}(s)+3 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{6}(s)} & {\Delta H=-1640.1 \mathrm{kJ}} \\ {\mathrm{P}_{4}(s)+5 \mathrm{O}_{2}(g) \longrightarrow \mathrm{P}_{4} \mathrm{O}_{10}(s)} & {\Delta H=-2940.1 \mathrm{kJ}}\end{array}$$

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Key Concepts

Hess's Law

Hess's Law states that the overall enthalpy change for a chemical reaction is the sum of the enthalpy changes for the intermediate steps that lead to the final reaction, regardless of the pathway taken. This principle allows the calculation of the enthalpy change for a reaction by combining other reactions with known enthalpy changes.

Enthalpy Change Calculation

Calculating the enthalpy change of a reaction involves adding and subtracting known enthalpies of formation or reaction according to the way individual reactions combine to yield the overall reaction. This method uses the fact that enthalpy is a state function, so the sum of the enthalpy changes from individual reactions gives the enthalpy change of the net reaction.

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