Calculate the energy change for the reaction Fe2 O3(s)+CO(g) ⟶2 FeO(s)+CO2(g) from the following

step 1 Fe2 .03 reacts with carbon monoxide to give us iron and CO2. Delta H is negative 23 kilojoules.

Calculate the energy change for the reaction Fe2 O3(s)+CO(g)...

Calculate the energy change for the reaction $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g)$ from the following: $$ \begin{array}{ll} \mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g) & \Delta H=-23.4 \mathrm{~kJ} \\ \mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) & \Delta H=-10.9 \mathrm{~kJ} \end{array} $$

Calculate the energy change for the reaction $\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+\mathrm{CO}(g) \longrightarrow 2 \mathrm{FeO}(s)+\mathrm{CO}_{2}(g)$ from the following:
$$
\begin{array}{ll}
\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g) & \Delta H=-23.4 \mathrm{~kJ} \\
\mathrm{FeO}(s)+\mathrm{CO}(g) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}_{2}(g) & \Delta H=-10.9 \mathrm{~kJ}
\end{array}
$$

Key Concepts

Hess's Law

Hess's Law states that the total enthalpy change of a reaction is independent of the pathway between reactants and products. This principle allows us to calculate the enthalpy change for any reaction by algebraically adding the enthalpy changes of several other reactions that sum to the overall reaction.

Reaction Enthalpy

Reaction enthalpy refers to the heat absorbed or released during a chemical reaction at constant pressure. It provides a quantitative measure of the energy change associated with the formation and breaking of chemical bonds, and is fundamental to understanding energy flow in chemical processes.

Thermochemical Equation Manipulation

Manipulating thermochemical equations involves reversing, scaling, or adding reactions to obtain a desired overall reaction. When reactions are reversed, the sign of the enthalpy changes is also reversed, and when they are scaled by a factor, the enthalpy change is multiplied by that factor. This method is essential for using known reactions to calculate the enthalpy change of an unknown reaction.

Combining Thermochemical Equations

By combining thermochemical equations, one can achieve cancellation of common intermediate species to yield the overall reaction equation. The overall enthalpy change is then the sum of the enthalpy changes of the individual equations. This approach reinforces the principle of energy conservation and enables the calculation of reaction enthalpies indirectly.

Transcript

00:18 Fe2 .03 reacts with carbon monoxide to give us iron and co2.

00:47 Delta h is negative 23 kilojoules.

00:56 I am going to multiply this equation by 3, and that will help me down the road.

01:05 So that gives a coefficient of 3, changes that to 6 iron, that to 9, co2, delta h is now negative 69.

01:18 Our next equation is iron 4 oxide, reacting with co2, to give us iron 3 oxide plus carbon monoxide.

01:56 And delta h is positive 39, but i switched this equation.

02:04 So originally the products were the reactants, and originally delta h was a negative.

02:13 At this point, i can cancel out a few things.

02:17 I can cancel out one of my co2s, so that leaves me with eight co2s up here.

02:25 I can cancel out one of my carbon monoxide.

02:28 That leaves me with two carbon monoxides here.

02:33 And i can cancel out the three fe2.

02:37 That's why i multiplied by 3 in the original equation.

02:44 So at this point, we've got fe 304 plus 2 co, yielding 6 iron, and 8 co2.

03:00 The next equation is 2fe 304 plus 8 coo, that gives us, i'm sorry, this is 2fe 304, plus 8 coo, that gives us, i'm sorry, this is this is what our current equation looks like after those original crossouts.

03:45 And so delta h here at this point is negative 39.

04:00 All right...

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