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Part A What must be the temperature if the following reaction has ΔG0= -44.0 kJ , ΔH0=-24.8 kJ, and ΔS0=15.2 JK−1?

Part A
What must be the temperature if the following reaction has ΔG0= -44.0 kJ , ΔH0=-24.8 kJ, and ΔS0=15.2 JK−1?
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

Answer 1

Natalie Anton

#T\approx1260K#

#\DeltaH°=\DeltaG°-T\DeltaS°# #-24.8kJ=-44.0kJ-T(15.2\times10^(-3)J/K)# #T\approx1260K#

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Answer 2

Mateo Aguilar

Use the Gibbs-Helmholtz equation: ΔG = ΔH - TΔS Rearrange for temperature (T): T = (ΔH - ΔG) / ΔS Substitute values: T = (-24.8 kJ - (-44.0 kJ)) / 15.2 JK^-1 Calculate the temperature.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

Part A What must be the temperature if the following reaction has ΔG0= -44.0 kJ , ΔH0=-24.8 kJ, and ΔS0=15.2 JK−1?

Part A What must be the temperature if the following reaction has ΔG0= -44.0 kJ , ΔH0=-24.8 kJ, and ΔS0=15.2 JK−1? Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

Part A
What must be the temperature if the following reaction has ΔG0= -44.0 kJ , ΔH0=-24.8 kJ, and ΔS0=15.2 JK−1?
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)