Substance: AH (kJ-mol¹¹) So (J.K¹-mol-¹) Use the data shown below, to calculate AH°rxn and AS°rxn at 25°C for the following reaction: 2 KCIO,(s) Which of the following statements is true about this reaction at standard state conditions? KCIO(s) -397.7 143.1 KCI(s) -436.5 82.6 O₂(g) 0 205.2 → 2 KCl(s) + 3 O₂(g) A) The reaction is only nonspontaneous above its equilibrium temperature. B) The reaction is nonspontaneous at all temperatures. C) The reaction is spontaneous at all temperatures. D) The reaction is only spontaneous above its equilibrium temperature? E) None of these.
Substance: AH (kJ-mol¹¹) So (J.K¹-mol-¹) Use the data shown below, to calculate AH°rxn and AS°rxn at 25°C for the following reaction: 2 KCIO,(s) Which of the following statements is true about this reaction at standard state conditions? KCIO(s) -397.7 143.1 KCI(s) -436.5 82.6 O₂(g) 0 205.2 → 2 KCl(s) + 3 O₂(g) A) The reaction is only nonspontaneous above its equilibrium temperature. B) The reaction is nonspontaneous at all temperatures. C) The reaction is spontaneous at all temperatures. D) The reaction is only spontaneous above its equilibrium temperature? E) None of these.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Substance:
AHof (kJ.mol-¹)
Sº (J.K-¹.mol-¹)
Use the data shown below, to calculate AH°rxn and AS°rxn at 25°C for the
following reaction:
2 KCIO,(s) 2 KCl(s) + 3 O₂(g)
Which of the following statements is true about this reaction at standard state
conditions?
KCIO3(s)
-397.7
143.1
KCI(S)
-436.5
82.6
O₂(g)
0
205.2
A) The reaction is only nonspontaneous above
its equilibrium temperature.
B) The reaction is nonspontaneous at all
temperatures.
C) The reaction is spontaneous at all
temperatures.
D) The reaction is only spontaneous above its
equilibrium temperature?
E) None of these.
Expert Solution
Step 1: Basic Concept and Formula
∆°Hrxn = Σni∆H°f(Product) - Σni∆H°f(Reactant)
Where, ni and ∆°Hf are stoichiometric coefficients and Standard enthalpy of formation of respective reactant and product.
∆°Srxn = ΣniS°(Product) - ΣniS°(Reactant)
Where, ni and S° are stoichiometric coefficients and Standard molar entropies of respective reactant and product.
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