### Spontaneity of a Chemical ReactionA chemical reaction has the following thermodynamic parameters:- **ΔH° (Enthalpy change)** = 100 kJ/mol- **ΔS° (Entropy change)** = 250 J/mol·KThe problem posed is: - **Question**: Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?### ExplanationTo determine if a reaction is spontaneous, we use the Gibbs free energy equation:\[ \Delta G° = \Delta H° - T \Delta S° \]Where:- \(\Delta G°\) is the change in Gibbs free energy.- \(\Delta H°\) is the change in enthalpy.- \(T\) is the temperature in Kelvin.- \(\Delta S°\) is the change in entropy.A reaction is spontaneous if \(\Delta G° < 0\).### Step-by-Step Solution1. **Convert Units:** Make sure that the units for ΔH° and ΔS° are compatible. ΔS° is given in J/mol·K, while ΔH° is in kJ/mol. Convert ΔH° to J/mol: \[ \Delta H° = 100 \text{ kJ/mol} \times 1000 \text{ J/kJ} = 100,000 \text{ J/mol} \]2. **Set Up Gibbs Free Energy Equation:** Substitute the values into the equation \(\Delta G° = \Delta H° - T \Delta S°\): \[ \Delta G° = 100,000 \text{ J/mol} - T \times 250 \text{ J/mol·K} \]3. **Determine Spontaneity at Room Temperature:** Assume room temperature is approximately 298 K. Substitute T = 298 K into the equation: \[ \Delta G° = 100,000 \text{ J/mol} - 298 \text{ K} \times 250 \text{ J/mol·K} \] \[ \Delta G° = 100,000 \text{ J/mol} - 74,500 \text{ J/mol} \] \[ \Delta G° = 25,500 \text{ J/mol} \] Since \(\Delta G° >

Answered: Image /qna-images/answer/f8d93ced-a881-4940-bc01-9076ae9af454.jpg

Answered: A reaction has AH°= 100 kJ/mol and AS°=…

A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, unde what temperature conditions will it become spontaneous?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

17. For the reaction: A + B C AH°= +45 kJ/mol and AS° = +60 J/K.mol. At what temperature will this reaction be spontaneous? * O The reaction is nonspontaneous at all temperatures. O At a temperature greater than 477 °C. O The reaction is spontaneous at all temperatures. O At a temperature greater than 750 °C. O At a temperature lower than 477 °C.
The reaction, Fe203(s) + 3C(s) → 2Fe(s) + 3CO(g) AH° = +490.7 kJ, AS° = +541 J-K-1 %3D This reaction is spontaneous only below a certain temperature always spontaneous never spontaneous spontaneous only above a certain temperature
10. What is the relationship between the following two compounds? (see attached screenshot). a. constitutional isomers b. stereoisomers c. identical d. not isomers; different compounds entirely
For a particular reaction, AH° = -93.8 kJ and AS° = –156.1 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? T = K Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculated temperature? less than greater than
For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?
49.For the decomposition of hydrogen peroxide to water and oxygen, H2O2(g) ⟶⟶ H2O(g) + O2(g) ΔΔH° = -106 kJ, and ΔΔS° = +0.0580 kJ/K. In what temperature range is the reaction spontaneous (ΔΔG° < 0)? A. The temperature must be greater than 1.83××103 K B. The temperature must be less than 1.83 ××103 K. C. The temperature must be between 225 K and 1.83 ××103 K. D. ΔΔG° is always less than zero. E. ΔΔG° is never less than zero.
51
A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous? 626.4 K This reaction is always spontaneous 498.3 K 434.6 K This reaction is never spontaneous
Which are spontaneous at all temperatures? Choose one or more: 2H,0(g) + SO,(g) - 152.4 J/K 2H,S(g) +30,(g) AH°. rxn = - 1037 kJ, AS°. rxn → 2SO3(g) - 197.8 kJ, ASº. 2SO,(g) +O2(g) AH°. rxn - 187.8 J/K rxn O so,(8) + H,0(1) → H,SO4(1) AH°. rxn - 132.5 kJ, AS° - 169.9 J/K rxn S(g) +O2(8) –→ SO,(g) - 574.0 kJ, AS°, ΔΗ. rxn - 124.6 J/K rxn none of the above