2. The enthalpy and entropy change of a reaction are -3.9 kJ/mole and +56.6 J/mole K respectively at 25o C. What is the free energy change in kJ/mole? Is this reaction always spontaneous, never spontaneous or does it depend on the temperature?

2. The enthalpy and entropy change of a reaction are -3.9 kJ/mole and +56.6 J/mole K respectively at 25o C. What is the free energy change in kJ/mole? Is this reaction always spontaneous, never spontaneous or does it depend on the temperature?

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

Related questions

Q: Calculate ΔGo for the following reaction at 25oC. C2H4(g) + O2(g) ----> CO2(g) H2O(g)…

Q: A chemical reaction has a standard entropy change, ΔSo, of -287.8 J/(molK) and a standard enthalpy…

A: The given data you have - ΔSo = -287.8 J/K-mol ΔHo = -138.1 kJ/mol

Q: What is the entropy change for the universe, delta Suniv, for the vaporization of one mole of CH3OH…

A: The solution is as follows :

Q: 50. For the process O2(g) → 2 O(g), AH° = +498 kJ. What would be predicted for the sign of ASrxn and…

A: 50. The given process has a positive sign for enthalpy change. Hence, the process will be an…

Q: the following reaction 2 NO (g) + O2 (g) -> 2 NO2 (g) Horxn = -12 kJ and Sorxn = -146 J/K. a.…

A: Given-> 2NO(g) + O2(g) ---> 2NO2(g) ∆H°rxn = -12 KJ = -12000 J (1 KJ = 1000J) ∆S°rxn = -146J/K…

Q: Consider the following reaction at 25°c: 2NH,(g)+CO,(g) =NH,CONH,(aq) + H,0(8) For this reaction A…

Q: For each reaction with ΔH = + 187 kJ/mol and ΔS = + 365 J/molK ,at what temperature at which the…

A: Given: ΔH = +187 KJ/mol or +187000 J/mol ΔS = +365 J/molK We have to calculate temperature(T) at…

Q: Have each group member look up ΔH °f and S° for one substance in the reaction: 3 O2( g) + 6 H2(g) +…

A: The enthalpy of a reaction is equal to the difference of the sum of the enthalpies of the product…

Q: For each reaction, calculate AHrn, ASn, and AGxn at 25 °C and state whether or not the reaction is…

A: a. The reaction: N₂O₄(g) → 2 NO₂(g) Standard enthalpies of formation: N₂O₄(g): Hf =…

Q: Consider the reaction: H2S(g)+SO2(g)---> 3S(g)+2H2O(l) for which delta H is -233 kJ and delta S…

A: Given:

Q: Consider this reaction: N2 (s) + 2 02 (g)→ 2NO2 (g) AS° = -121.77 J/K.mol; AH° = %3! 66.36 kJ/mol…

A: From the given question it is given that, ΔSo < 0 ΔH0 > 0

Q: 10. Determine whether or not the following reaction is spontaneous under standard conditions from…

A: Step 1: Step 2:Step 3: Step 4:

Q: For the following endothermic reaction, predict under which conditions the reaction will be…

A: The spontaneous nature of a system can also be predicted by the Gibbs free energy change of the…

Q: 9. A chemical reaction under standard state has the enthalpy of reaction: A,H° = +117 kJ and the…

A: B) The reaction is entropy driven.

Q: 2. Consider the following reaction at 298 K: N2 04(8) = 2NO2(g) Kp = 0.142 What is the standard free…

Q: free

Q: 12. Consider the reaction H₂(g)+ S(s)→ H₂S(g) for which AH = -20 kJ and AS - +43] Kat 298.15 K.…

A: Given here a reaction with its enthalpy change and entropy change valuesat 298.15 K. We are asked to…

Q: For the following reaction, AH° for the reaction is -206.1 kJ/mol, while AS° is -215 JK•mol. NO (g)…

A: The reaction given in the question is given as - NO (g) + 1/2 Cl2 (g) → NOCl (g) The standard change…

Q: [1] Given: CH«(g) + H2O(g) – CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is…

A: 1. Given : CH4(g) + H2O(g) → CO(g) + 3H2(g) ∆H° = +206.1 kJ/mol ∆S° = +215 J/K.mol T = 25°C To…

Q: 17. For the reaction: A + B → C AH°= +300 kJ/mol and AS° = +200 J/K.mol. At what temperature will…

A: Given, ∆H° = 300kJ/mol ∆S° = 200J/K.mol

Q: Consider the following thermochemical equation: H2O2(1) H2O(1) + %02(g) AH= -98.2 kJ When is this…

Q: Given the following data, predict whether the reaction below is spontaneous at 25°C: NO2(9) + N20(9)…

A: The given reaction is as follows: NO2(g) + N2O(g) →3NO(g) The ∆rG° of the reaction can be calculated…

Q: Consider the information below about a given hypothetical reaction. Which statement is true? AHO…

A: The reaction is said to be spontaneous if the change in Gibbs free energy change () is negative. The…

Q: 3. The equilibrium constant for the reaction: 250:(8) + O:(8) = 250,(8) is 2.8 x 10' at 25.0°C. a.…

A: Given, reaction : 2SO2(g) +O2(g)⇌2SO3(g) Equilibrium constant , Keq=2.8×102

Q: For the reaction below, which statement best describes what is happening with the sign of AGO? 2 Cu…

A: In this reaction change in entropy is negative beacuse no of particle decreasing And ∆H is negative…

Q: If the Delta*H = 135kJ / m * ol and AS 92 J/K mol, at what temperature does this reaction become…

Q: Use the AH°f information provided in the table below to calculate AH°rxn for the following reaction.…

Q: The enthalpy and entropy changes for a reaction at 298 K are ∆H = -102 kJ and ∆S = -208 J/K. Which…

A: Given: ∆H = -105 kJ; ∆S = -208 J/K; T = 298 K∆G = ∆H-T∆S∆G = -105 kJ - (298 K) (-0.208…

Q: For each reaction, calculate AHan ASn and AGan at 25 "C and state whether or not the reaction is…

A: Standard heat of formation of N2O4 (ΔHfo) = 9.16 KJ/mol. Standard heat of formation of NO2 (ΔHfo) =…

Q: 57. For each reaction, calculate AHan, AS, and AGan at 25 °C and state whether or not the reaction…

A: Note - Since you have asked multiple questions (multiple reactions), we are supposed to solve only…

Q: calculate the free energy change (in kJ) of a reaction at 466.4K that has an entropy change of…

A: Given, ΔS = 692.2 J/K = 0.6922 kJ/K ΔH = - 4.24 kJ T = 466.4 K Free energy change ( ΔG )…

Q: Consider the reaction: 4 A (g) ------ 2 B (s) + 3 C (g) + 20.5 kJ, at what…

Q: When in 1 atm of pressure, when is the reaction of formation of ozone from oxygen spontaneous? 3 O2…

A: We have to tell given reaction is spontaneous or not

Q: Consider the following reaction in which acetic acid decomposes to form methane and carbon dioxide:…

Q: The following reaction is spontaneous at room temperature.

A: Since we know that a spontaneous reaction is the reaction which occurs on it own without any outside…

Q: For the process O2(g) 2O(g), ΔH° = 498 kJ·mol –1. What would be the predicted sign of ΔS°rxn…

A: Given that :Reaction = O2(g) → 2O(g) ∆H° = 498kJ/mol

Q: ΔH° = -90.84 kJ for the following reaction: 2 Hg(l) + O2(g) →2 HgO(s). This reaction is most likely…

A: Given that, A reaction, 2 Hg(l) + O2(g) →2 HgO(s) ΔH° = -90.84 kJ

Q: Given the thermodynamics data for the following substances:…

A: Gibbs free energy is the free energy in the system that is used to do some useful work. It is…

Q: For the reaction below, which statement best describes what is happening with the sign of AGO? NagP…

A: the reaction given is exothermic that means the change in enthalpy is -ve . now the entropy change…

Q: For the reaction 2NH3(g) + 3N,0(g)- →4N2(g) + 3H,0(g) AH° = -879.5 kJ and AS° = 288.1 J/K The…

A: Gibb's equation can be written as, ∆G°=∆H°-T∆S° Where, ∆G°= change in free energy ∆H°= change in…

Q: What is true about 02 (g) + 2HCl (g) AHY-48 kJ mol i. The reaction is non-spontaneous. ii. The…

A: Option i is correct.This is due to the fact that negative ∆G results in an spontaneous…

Q: O The reaction is never spontaneous. O The reaction is only spontaneous at high temperatures. The…

Q: What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 342.26…

Question

T SUMMATIVE TEST (GENERAL CHEMISTRY 2-2 OT)
A. Given the equation, calcite the standard free energy change. Answer what is being asked?

2. The enthalpy and entropy change of a reaction are -3.9 kJ/mole and +56.6
J/mole K respectively at 250 C. What is the free energy change in kJ/mole?
Is this reaction always spontaneous, never spontaneous or does it depend on
the temperature?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

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 free energy change is related to the enthalpy change and the entropy change: ΔG = ΔH – T ΔS. What is ΔS for reaction 3? Question 8 options: –200 J mol–1 K–1 400 J mol–1 K–1 200 J mol–1 K–1
For the reaction of gaseous substances with increasing gaseous molecules (from reactant to product side) and given the ΔH° that is +150 kJ/mol and ΔS° that is +171 J/K ∙ mol, how can you describe this reaction? a. It is spontaneous only at low temperatures. b. It is spontaneous only at high temperatures. c. It is spontaneous all the time. d. It is non-spontaneous.
a. H₂O b. SH- c. S²- BH3 e. NH3 14. At what temperatures will a reaction be spontaneous if A,H=+117 kJ and A,S = -35 J/K? The reaction will be spontaneous at any temperature. b. The reaction will never be spontaneous. c. Temperatures between 12.7 K and 135 K d. All temperatures above 94.1 K e. All temperatures below 94.1 K
For each reaction with ΔH = + 245 kJ/mol and ΔS = + 48 J/molK ,at what temperature at which the reaction will be spontaneous.
C3H8 (g) + 502 (g) --> 3CO2 (g) + 4H2O (g) + 2200 k) Given the above equation, which statement is correct? A. can be spontaneous at all temperatures B. can be spontaneous at high temperatures O C. can be spontaneous at low temperatures D. can be spontaneous at no temperatures
The following reaction is endothermic. 2NH3(g) → N2(g) + 3H2(g) This means the reaction A. will be spontaneous at high temperatures. B. will be spontaneous at low temperatures. C. is not spontaneous at any temperature. D. is spontaneous at all temperatures.
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.
For each reaction, calculate ΔH°rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 °C?a. 2 CH4( g)------->C2H6( g) + H2( g)b. 2 NH3( g)------> N2H4( g) + H2( g)c. N2( g) + O2( g)-------->2 NO( g)d. 2 KClO3(s)-------->2 KCl(s) + 3 O2( g)
4
A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
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