For the reaction FeCO3(s)⟶FeO(s)+CO2(g);ΔH=82.8kJ at 25∘C what is (ΔE or ΔU) at 25"C?

ΔH=ΔE+ΔngRT⇒ 82.8=ΔE+1×8.314×2981000⇒ ΔE=80.32

For the reaction FeCO3(s)⟶FeO(s)+CO2(g);ΔH=82.8kJ at 25∘C what is (ΔE or ΔU) at 25"C?

ΔH=ΔE+ΔngRT⇒ 82.8=ΔE+1×8.314×2981000⇒ ΔE=80.32

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For the reaction ${FeCO}_{3} (s) ⟶ FeO (s) + {CO}_{2} (g); ΔH = 82 .8 kJ at 25^{\circ} C$ what is $(ΔE or ΔU)$ at 25"C?

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85.28 kJ

-2394.77 kJ

30.32 kJ

82.8 kJ

answer is B.

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Detailed Solution

$\begin{array}{l} ΔH = ΔE + {Δn}_{g} RT \\ \Rightarrow 82 .8 = ΔE + \frac{1 \times 8 .314 \times 298}{1000} \\ \Rightarrow ΔE = 80 .32 \end{array}$

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For the reaction FeCO3(s)⟶FeO(s)+CO2(g);ΔH=82.8kJ at 25∘C what is (ΔE or ΔU) at 25"C?

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For the reaction ${FeCO}_{3} (s) ⟶ FeO (s) + {CO}_{2} (g); ΔH = 82 .8 kJ at 25^{\circ} C$ what is $(ΔE or ΔU)$ at 25"C?