### Educational Content on Spontaneity of Chemical Reactions**Question 8****Show why reaction (b) is spontaneous only at low temperature, while reaction (a) is always non-spontaneous.****Reactions:**a) \( \text{CH}_4(g) + 2\text{O}_2(g) \rightarrow 2\text{H}_2\text{O}(l) + \text{CO}_2(g) \) (endothermic)b) \( 2\text{C}_2\text{H}_6(g) + 7\text{O}_2(g) \rightarrow 6\text{H}_2\text{O}(l) + 4\text{CO}_2(g) \) (exothermic)### Detailed Explanation**a) Endothermic Reaction:**In the above reaction (a), methane (CH₄) reacts with oxygen (O₂) to form water (H₂O) and carbon dioxide (CO₂). Since this reaction is endothermic, it requires the absorption of heat. For an endothermic reaction, ΔH (change in enthalpy) is positive. Endothermic reactions are usually non-spontaneous because they need continuous energy input to proceed.**b) Exothermic Reaction:**In reaction (b), ethane (C₂H₆) reacts with oxygen (O₂) to yield water (H₂O) and carbon dioxide (CO₂). This is an exothermic reaction, meaning it releases heat into the surroundings. Here, ΔH is negative. However, even exothermic reactions can be non-spontaneous if the temperature conditions are not favorable. Reaction (b) is spontaneous only at low temperatures because low temperatures favor exothermic processes.### Key Concepts- **Spontaneity:** A spontaneous reaction occurs naturally under given conditions. It depends on the changes in enthalpy (ΔH) and entropy (ΔS) of the system, and the temperature (T) as per the Gibbs free energy formula: \[ \Delta G = \Delta H - T\Delta S \] A reaction is spontaneous if ΔG (change in Gibbs free energy) is negative.- **Endothermic Reactions:** Typically require heat absorption from the surroundings. These reactions are often non-spontaneous because

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A Moving to another question will save this response. Question 8 Show why, reaction (b) is spontaneous only at low temperature, while reaction (a) is always non-spontaneous. a) CH4(g) + 202(g) -> 2H2O(l) + CO2(g) (endothermic) b) 2C2H6(g) + 702(g) -> 6H2O(l) + 4CO2(g) (exothermic) For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). Av I Arial V 14px

A Moving to another question will save this response. Question 8 Show why, reaction (b) is spontaneous only at low temperature, while reaction (a) is always non-spontaneous. a) CH4(g) + 202(g) -> 2H2O(l) + CO2(g) (endothermic) b) 2C2H6(g) + 702(g) -> 6H2O(l) + 4CO2(g) (exothermic) For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). Av I Arial V 14px

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...

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12) Calculate AG°pm for the following reaction at 25.0 °C. Is the reaction spontaneous? 3 H2 (g) + N2 (g) 2 NH3 (g) Substance AH°t (kJ/mol) AG°r (kJ/mol) S (J/mol K) H2 (g) 130.7 N2 (g) 0. 191.6 NH3 (g) -45.9 -16.4 192.8
8e. Consider the following reaction: Caco3 (s) → Cao (s) + CO2 (g) Data: A,H = +177.5 kJ mol1 A,S = +160.7 J mol1K1 At which temperature will the reaction become spontaneous?
The standard reaction free energy AG=-1482. kJ for this reaction: 4 Fe(s) + 30₂(g) 2 Fe₂O3(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. reaction 2Fe₂O₂ (s) 4Fe(s) + 30, (g) - Fe(s) + O₂(g) → Fe₂03 (s) Fe₂O₂ (s) → Fe(s) + 0₂ (8) AG kJ kJ X 5
Is this reaction spontaneous? Why or Why not? CaC2(s) + 2H2O(l) ---> C2H2(g) + Ca(OH)2(s) Delta H(rxn)= -128.9kJ Substances: CaC2(s)= S(1/mol*K)= 70.0 Delta H(f) (kJ/mol)= -59.8 H20(l)= S= 69.9 Delta H= -285.8 C2H2(g)= S= 200.8 Delta H= ? Ca(OH)2= S= 83.4 Delta H= -986.1
Please help with # 39. I do not know how to solve
2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K. Is the reaction endothermic (+ΔH) or exothermic (-ΔH)?
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
5-For the reaction, A+B C, AH-+30 kJ; AS°=+50 J/K.Therefore the reaction is: (a) spontaneous at all temperatures. (b) nonspontaneous at all temperatures. (d) irreversible at all temperatures (c) reversible at all temperatures 6- How much heat is necessary to convert 2mol of water at( 50°C) to steam at 150°C?The molar heat capacity of liquid water and steam are 75.3 J/mol. K and 36.4 J/mol. K respectively. The heat of vaporization 40.7 KJ/mol. a-81400J 7- From the reactions: b-82.337KJ c-753J d-3641 e- none of them Cgraphia +2H2(g) → CHA(R) AH = -79.9KJ C(graphia + 2Cl2(g) → CCla AH = -139KJ H 20 + Cl₂00) → HCL) AH-92.3KJ 202) calculate AH, for the reaction CH ACE +4Cl2) a- (-615.1KJ) c-(-428.3KJ) 4HCI+CCI b-(-311.2KJ) d- none of them
Determine whether the following reactions are spontaneous or non-spontaneous. a) N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g), ΔG = -32,960 J b) 2 NH3 (g) ⟶ N2 (g) + 3 H2 (g), ΔG = 32,960 J HINT: The change in free energy (ΔG) for reaction is equal to the difference in free energy between the products (Gproducts) and the reactants (Greactants): ΔG = (Gproducts) - (Greactants) In spontaneous reactions, the free energy of the products (Gproducts) of a reaction is less than the free energy of the reactants (Greactants). When this is the case, will the change in free energy (ΔG) will have a negative value or a positive value?
What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C8H8(g)) = 345.2600J/mol*K and the heat of formation of C8H8(g)) is 147.8500 kJ/mol?C8H8(g) ↔ 8C(gr) + 4H2(g)a)661.88 Kb)707.958 Kc)the reaction is never spontaneousd)the reaction is always spontaneous
Spontaneous or non-spontaneous
6. For each reaction below, determine the sign of AH and AS. Also state under what conditions the reaction is spontaneous (in the forward direction): (a) never spontaneous, (b) always spontaneous, (c) spontaneous at low temperatures, or (d) spontaneous at high temperatures. 1) C2 (g) → 2 Cl (g) (ii) 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g)