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I the AGⓇ of the reaction ABS. 56 kJ/mol which of the following statements are correct?...
PLEASE EXPLAIN WHY EACH ANSWER IS TRUE OR FALSE 6. The standard free energy AG° of...
PLEASE EXPLAIN WHY EACH ANSWER IS TRUE OR FALSE
6. The standard free energy AG° of the reaction A +B C following statements true or false. D is +3 kJ/mol. Mark the The standard free energy of the reaction can be calculated from the free energies of formation of A, B, C, and D from the elements. The reaction is endothermic under standard state conditions. One way to get the reaction to proceed to the right is to increase the...
- (3p total Free energy of a chemical reaction is related to the equilibrium constant a....
- (3p total Free energy of a chemical reaction is related to the equilibrium constant a. Write the equation relating K and G. AG - K-AST b. For a reaction to proceed spontaneously from right to left, the value of K must be greater than I or less than 1. (Circle your answer). c. For a reaction to proceed spontaneously from right to left, the change in free energy must be greater than 0 or less than 0. (Circle your...
11. Consider the following reaction with the equilibrium concentrations written below at 25°C. You notice that...
11. Consider the following reaction with the equilibrium concentrations written below at 25°C. You notice that entropy has increased so it is possible this is a spontaneous reaction in the forward direction. However, you do not have information about the enthalpy of reaction so you cannot use AG AH-TAS to check. You are only given the concentrations of the reactant and product at equilibrium. Show mathematically whether the reaction is spontaneous Ad 7 2B Equilibrium concentrations 10.112] (0.189)
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following...
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following equilibrium system sscc Fe(a)SCNag) FeSCNP(o) The equilibrium constant, K of this system is (2) resCN KTeSCN Finding K for this system using a colouurimeter and absorhance values has already been described in the "Determination of an Equilibrium Constant" experiment. A similar method is used in this experiment, but the temperature is varied so give values of the equilibrium constant at different temperatures. From the...
Thermodynamic data is available for each of the following dissolution reactions (solids dissolving in water) at...
Thermodynamic data is available for each of the following dissolution reactions (solids dissolving in water) at standard conditions at 25 degree C. Recall that standard conditions mean that all concentrations are 1 M a. Which of the solids will dissolve spontaneously at standard conditions? Are any of them near equilibrium? What leads you to your conclusions? b. Which of the solids will not dissolve at standard conditions? c. Are any of the dissolutions entropy driven? Enthalpy driven? Which? Explain. d....
the correct answer to #11 is supposed to be b but i keep getting c. what...
the
correct answer to #11 is supposed to be b but i keep getting c.
what am i doing wrong? also, the correct answer to #14 is b but i
keep getting d. please explain where i am going wrong. thank
you
11. Consider the reaction in the previous question, what the equilibrium constant would be equal to at 25°C? a) 0.645 AGE-RT enk b) 1.03x10-16 c) 9.64x10-1. 91.2-0008314 (298,15) enk d) 7.03x108 -0.036B-Ink 12. When a reaction is found...
+ Consider the following hypothetical reaction (at 305 K). Standard free energies, in kJ/mol, are given...
+ Consider the following hypothetical reaction (at 305 K). Standard free energies, in kJ/mol, are given in parentheses. A B с AGⓇ = ? (-32.9) (207.8) (-237.0) What is the value of the equilibrium constant for the reaction at this temperature? Answer:
Which of the following statements is true for the product-favored reaction shown at 25ºC ? A(g) ...
Which of the following statements is true for the product-favored reaction shown at 25ºC ? A(g) ---> B(g) ΔH = - 20 kJ/mole ΔS = - 26 J/mole•K the reaction is enthalpy and entropy driven this reaction is at equilibrium at 25ºC the reaction is entropy driven the reaction is enthalpy driven In the reaction, the overall entropy change for the universe is negative
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The...
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The bond dissociation energy for bond breaking is always negative. C) Bond making is exothermic. D) The bond dissociation energy for bond formation is always negative. 37. Using the bond dissociation energies given, calculate AH® for the following reaction. CH,CH -Br + H2O CH,CH-OH + HBr AH KJ/mol Bond A-B CH3CH2-Br H-OH сHCH-он H-Br A) +108 KJ/mol B) -130 KJ/mol C) -22 KJ/mol D) +22...
(a) Calculate ?G for the reaction: 2H,000 H()+OH (ag) at 25 C given the following initial...
(a) Calculate ?G for the reaction: 2H,000 H()+OH (ag) at 25 C given the following initial concentrations. HO] 1.0x 10-12 M and (OH]- 20 x10* M (b) Predict the direction in which the reaction will proceed spontaneously to establish equilibrium. 10. The AG° for the reaction: N,(g)+3H,(g)0 2NH,(g) is 33.3 kJ/mol at 25°C. What is the value of Kp?
PLEASE EXPLAIN WHY EACH ANSWER IS TRUE OR FALSE
6. The standard free energy AG° of the reaction A +B C following statements true or false. D is +3 kJ/mol. Mark the The standard free energy of the reaction can be calculated from the free energies of formation of A, B, C, and D from the elements. The reaction is endothermic under standard state conditions. One way to get the reaction to proceed to the right is to increase the...
- (3p total Free energy of a chemical reaction is related to the equilibrium constant a. Write the equation relating K and G. AG - K-AST b. For a reaction to proceed spontaneously from right to left, the value of K must be greater than I or less than 1. (Circle your answer). c. For a reaction to proceed spontaneously from right to left, the change in free energy must be greater than 0 or less than 0. (Circle your...
11. Consider the following reaction with the equilibrium concentrations written below at 25°C. You notice that entropy has increased so it is possible this is a spontaneous reaction in the forward direction. However, you do not have information about the enthalpy of reaction so you cannot use AG AH-TAS to check. You are only given the concentrations of the reactant and product at equilibrium. Show mathematically whether the reaction is spontaneous Ad 7 2B Equilibrium concentrations 10.112] (0.189)
STANDARD ENTHALPY AND ENTROPY CHANGES OF A REACTION INTRODUCTION (1) Part 3, Mes Consider the following equilibrium system sscc Fe(a)SCNag) FeSCNP(o) The equilibrium constant, K of this system is (2) resCN KTeSCN Finding K for this system using a colouurimeter and absorhance values has already been described in the "Determination of an Equilibrium Constant" experiment. A similar method is used in this experiment, but the temperature is varied so give values of the equilibrium constant at different temperatures. From the...
Thermodynamic data is available for each of the following dissolution reactions (solids dissolving in water) at standard conditions at 25 degree C. Recall that standard conditions mean that all concentrations are 1 M a. Which of the solids will dissolve spontaneously at standard conditions? Are any of them near equilibrium? What leads you to your conclusions? b. Which of the solids will not dissolve at standard conditions? c. Are any of the dissolutions entropy driven? Enthalpy driven? Which? Explain. d....
the
correct answer to #11 is supposed to be b but i keep getting c.
what am i doing wrong? also, the correct answer to #14 is b but i
keep getting d. please explain where i am going wrong. thank
you
11. Consider the reaction in the previous question, what the equilibrium constant would be equal to at 25°C? a) 0.645 AGE-RT enk b) 1.03x10-16 c) 9.64x10-1. 91.2-0008314 (298,15) enk d) 7.03x108 -0.036B-Ink 12. When a reaction is found...
+ Consider the following hypothetical reaction (at 305 K). Standard free energies, in kJ/mol, are given in parentheses. A B с AGⓇ = ? (-32.9) (207.8) (-237.0) What is the value of the equilibrium constant for the reaction at this temperature? Answer:
6. Which of the following statements is not true? A) Bond breaking is endothermic. B) The bond dissociation energy for bond breaking is always negative. C) Bond making is exothermic. D) The bond dissociation energy for bond formation is always negative. 37. Using the bond dissociation energies given, calculate AH® for the following reaction. CH,CH -Br + H2O CH,CH-OH + HBr AH KJ/mol Bond A-B CH3CH2-Br H-OH сHCH-он H-Br A) +108 KJ/mol B) -130 KJ/mol C) -22 KJ/mol D) +22...
(a) Calculate ?G for the reaction: 2H,000 H()+OH (ag) at 25 C given the following initial concentrations. HO] 1.0x 10-12 M and (OH]- 20 x10* M (b) Predict the direction in which the reaction will proceed spontaneously to establish equilibrium. 10. The AG° for the reaction: N,(g)+3H,(g)0 2NH,(g) is 33.3 kJ/mol at 25°C. What is the value of Kp?
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