2Al(s) + 3C12(g) -> 2AICI3(s) The above reaction is not spontaneous under standard conditions, but becomes spontaneous as the temperature decreases. Which choice below is true at standard conditions? Ο Α. ΔΗ +, ΔS+ Ο Β. ΔΗ -, ΔS+ O C. AH +, AS O D. AH -, AS -

2Al(s) + 3C12(g) -> 2AICI3(s) The above reaction is not spontaneous under standard conditions, but becomes spontaneous as the temperature decreases. Which choice below is true at standard conditions? Ο Α. ΔΗ +, ΔS+ Ο Β. ΔΗ -, ΔS+ O C. AH +, AS O D. AH -, AS -

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: Sodium carbonate can be made by heating sodium bicarbonate: 2NaHCO3(s)→ Na2CO3(s) + CO2(g) + H₂O(g)…

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

Q: Consider the reaction in the previous problem H2O2 0 H20 + O2e) Is the reaction spontaneous or…

A: A spontaneous reaction is one which takes places on its own. For a spontaneous reaction, ∆G∘should…

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: 15) Consider the following reaction at 25°C. If the pressure of H2 is 1.00 atm, the pressure of N2…

Q: Below what temperature does the following reaction become spontaneous? FeO(s) + CO(g) → CO2(g) +…

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: Using the values provided in the table below, calculate ΔS for the following reaction: 3H2SO4(l) +…

A: Entropy represents the degree of randomness. And ΔS is the difference in entropy of products and…

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: = -255 kJ/mol and AS°rxn 211 J/mol at 55°C. Do you expect the °rxn to confirm your prediction. 2. A…

A: Spontaneous reaction :- A reaction which takes place on its own without the need of any external…

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: Which of the following changes will always be true for a spontaneous reaction? +ΔG –ΔG +ΔS…

A: The spontaneous reaction means the reaction which occur without intervenation at given set of…

Q: For each reaction, calculate ΔH °rxn, ΔS°rxn, and ΔG°rxn at 25 °C and state whether or not the…

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

Q: Pure crystalline silicon, Si (s), can be obtained by reacting silicon dioxide (in the crystalline…

A: The ∆H0 and ∆S0 of the reaction can be calculated as follows:

Q: Na (s) + 20 (g)-2NO; (e) AS = -121.77 J/K.mol; AH° = 66.36 kJ/mol Is the reaction shown above…

Q: For the conversion of reactant A to product B, the change in enthalpy is 7.80 kJ·mol-1 and the…

A: Solution: ∆H= 7.80 KJ mol-1∆S= 44.4 JK-1

Q: 4. For a chemical reaction to be spontaneous at all temperatures, which of the following conditions…

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

Q: Refer to Appendix B in your textbook entitled Standard Thermodynamic Values for Selected Substances…

A: Given: 2SO2(g) + O2(g) -----> 2SO3(g) From standard Table: ∆f H°(SO2(g)) = -296.8 kJ/mol ∆f…

Q: For a certain reaction, ΔH = -35.4 kJ/mol and ΔS = -85.5 J/K mol. Is this reaction endothermic or…

Q: A certain chemical reaction has a negative value for ΔStotal. What must be true? o The reverse…

A: The question is asking about the implications of a negative value for ΔStotal in a chemical…

Q: Predict the spontaneity of a reaction (and the temperature dependence of the spontaneity) for each…

Q: A

A: We Will Choose Correct option

Q: Use the tables in the text to determine whether each reaction is spontaneous under standard…

Q: Calculate ∆ Go For the following reaction at 150o C. Is it spontaneous as written? (Hint: need to…

Q: The graph below shows the change in Gibbs free energy for two reactions. Change in Gibbs Free Energy…

A: According to Thermodynamics, ∆G>0 = non spontaneous ∆G< 0 = spontaneous ∆G = 0 , At…

Q: Vhich of the following statements is TRUE regarding the spontaneity of the exothermic reaction isted…

A: Q. Which of the following statements is True regarding the spontaneity of the exothermic 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: 1. Determine whether the reaction below is spontaneous or non-spontaneous at 25°C. H2 + Cl2 → HCI…

A: Here we are required to predict whether the given reaction is spontaneous or non spontaneous

Q: For the reaction 2 NH3 (g) --> N2 (g)+ 3 H2 (g) , ∆H = +92 kJ. Which of the following is true?…

A: The given reaction is, 2 NH3 (g) --> N2 (g)+ 3 H2 (g) , ∆H = +92 kJ ∆H is positive, that means…

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

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: How does temperature affect the spontaneity of a system with AHsys > 0 and AS sys > 0. O The…

A: Given-> ∆Hsys > 0 ∆Ssys > 0

Q: Calculate Go for the following reaction at 25oC. What is k of reaction? What type of reaction is…

A: Well, we will first calculate the standard gibbs free energy of the reaction. For that first of all…

Q: Which one of the following reactions cannot proceed spontaneously as written at any temperature?…

A: Relation of ∆Hrxn and ∆Grxn The equation is ; ∆G=∆H-T∆S∆G=Gibb's free energy∆H=enthalpy of…

Q: A reaction is never spontaneous when A. O AS is positive surr B. O ASis negative surr C. O AS is…

A: ∆Suniverse = ∆Ssytem + ∆Ssurroundings

Q: Without doing any calculations, determine the sign of AS and ASu, for each chemical reaction. In…

A: In a thermodynamic system, the entropy of the system is defined as the randomness of the system.…

Q: If ΔH and ΔS for a reaction are both negative which of the following is true. Select one: a. It…

A: We know that ΔG =ΔH - TΔS WHERE ΔG= Gibbs Free Energy ΔH= Enthalpy ΔS = Entropy T= Temperature For…

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: For a given chemical reaction at a certain temperature, Q = K = 2.7 x 104. Which statements are true…

A: relation are

Q: 8. Gaseous nitrosyl bromide, NOBr, is formed by the reaction 2NO(g) + Br,(g)2 2NOB1(g) At 25°C, the…

A: Reaction quotient is the ratio of concentrations/ pressure of products to concentrations/pressure of…

Q: Is the formation of ozone (O3(g)) from oxygen (O2(g)) spontaneous at room temperature under standard…

A: Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and…

Q: For a particular reaction, AH° = 67.7 kJ and AS° = 126.9 J/K. Assuming these values change very…

Q: 2H2O(g) ----> 2H2(g) + O2(g) The reaction above is only spontaneous at temperatures above 2000K.…

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

Q: For a chemical reaction, ΔSrxn = –200 J/K, and ΔHrxn = –50 kJ at approximately 298 K. At what…

A: ∆Srxn = -200 J/K ∆Hrxn = -50KJ = -50000 J ( 1 KJ = 1000 J)

Q: In a biochemical reaction, A + B ® C with DG= 30 kJ/mol. Which of the following reactions, if any,…

A: A question based on chemical thermodynamics, which is to be accomplished.

Question

2Al(s) + 3C12(g)–> 2AIC13(s)
The above reaction is not spontaneous under standard conditions, but becomes spontaneous as the temperature decreases. Which choice below is true at standard
conditions?
Ο Α. ΔΗ+, Δ5+
O B. AH -, AS +
Ο C. ΔΗ+, ΔS
Ο D.ΔΗ-, ΔS-

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

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

Chemistry Above what temperature does the following reaction become non-spontaneous? 2 H₂S(g) + 3 O₂(g) → 2 SO₂(g) + 2 H₂O(g) AH = -1036 kJ; AS = -153.2 J/K O 158.7 K This reaction is nonspontaneous at all temperatures. O 298 K This reaction is spontaneous at all temperatures O 6.762 × 103 K
Consider the oxidation of elemental cadmium (II) oxide. 2Cd(s)+O2 (g)--> 2CdO(s) Using the following thermochemical data, calculate the minimu temperature in degrees Celsius at which this reaction is spontaneous. Species delta Hf degrees (kJ/mol) S degrees (J/molxK) Cd(s) 0 51.8 O2 0 205.2 CdO(s) -258.4 54.8 Select the correct answer: a. 2594 degrees Celsius b. 2321 degrees Celsius c. 1.278 degrees Celsius d. -271.9 degrees Celsius e. -270.6 degrees Celsius
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
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
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.
1. On the basis of your experience, predict which of the following reactions are spontaneous. 1) NaCl(s)→→ NaCl(/) at 25 °C 2) 2 NaCl(s)→→ 2 Na(s) + Cl₂(g) 3) CO2(g) → CO2(s) at 25 °C 4) CO2(g) → C(s) + O2(g) 5) H₂O(s)→ H₂O() at 25 °C a) 1, 2, and 3 b) 1, 2, and 4 c) 3 and 5 d) 3 e) 5
∆Gº for the reaction, H2(g)+Br2(g)⇄2HBr(g), is -33.3 kJ. Which statement below is true? To make this reaction go forward, 33.3 kJ must be added. This reaction is non-spontaneous. This reaction is spontaneous. This reaction cannot be at equilibrium.
If the process is exothermic and not spontaneous, then what must be TRUE? O a. AS0 O c. AH=0 O d. AS> 0
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)
Consider the reaction below for the decomposition of carbon tetrachloride gas: CCl4(g) ------> C(s) + 2Cl2 (g) ΔH = + 95.7 kJ; ΔS = + 142.2 J/K If the reaction above is not spontaneous at 25 oC, determine at what temperature (if any) the reaction becomes spontaneous.
The vaporization of compound A is described by the following chemical equation. A(1) A(g) AH vap (78.97 °C) = 37.87 kJ/mol Calculate the entropy of vaporization, A.Svap, for A(1) at 25.0 °C given that the boiling point of A is 78.97 °C, and the molar heat capacity of A(1) is 114.29 J/(mol K). Assume that the molar heat capacity of A(g) is 55.9% of that of A(1). ASvap = Calculate the standard enthalpy of vaporization, AHvap, for A(1) at 25.0 °C. AH vap = Calculate tl AG'vap = x10 TOOLS of vaporization, AGvap, at 25.0 °C. Determine the equilibrium constant K for the va 1970ea J. mol-1. K-1 kJ/mol kJ/mol