Consider the following reaction run at 25 °C: L (g) + Cl2 (g) = 2 ICI (g) a) A mixture at 25 °C containing I2 and Cl2 at a pressure of 0.125 atm and IC| at a pressure of 1.50 atm has DG=+1.41 kJ. Calculate the standard change in Gibbs free energy for this reaction and use the information to complete Part b) b) Fill in the blanks in the paragraph below. Write your answers in the boxes on your test template that correspond to the blanks in the paragraph. Under the specified conditions (P2 = Pcz = 0.125 atm and Pıa = 1.50 atm) at 25 °C, the value AG = +1.41 kJ indicates that this reaction will proceed in the (i) direction until a state of (ii) is reached and the value of AG = (iii) change has a (iv)_ (v)_ reaction will proceed in the (viii). (ix) value of (x). The standard free energy value, indicating that when Piz = - the %3D Pca = (vi)_ , and Pici = (vii)_ direction until AG = At that point, the standard free energy change will have a at 298 K.

Consider the following reaction run at 25 °C: L (g) + Cl2 (g) = 2 ICI (g) a) A mixture at 25 °C containing I2 and Cl2 at a pressure of 0.125 atm and IC| at a pressure of 1.50 atm has DG=+1.41 kJ. Calculate the standard change in Gibbs free energy for this reaction and use the information to complete Part b) b) Fill in the blanks in the paragraph below. Write your answers in the boxes on your test template that correspond to the blanks in the paragraph. Under the specified conditions (P2 = Pcz = 0.125 atm and Pıa = 1.50 atm) at 25 °C, the value AG = +1.41 kJ indicates that this reaction will proceed in the (i) direction until a state of (ii) is reached and the value of AG = (iii) change has a (iv)_ (v)_ reaction will proceed in the (viii). (ix) value of (x). The standard free energy value, indicating that when Piz = - the %3D Pca = (vi)_ , and Pici = (vii)_ direction until AG = At that point, the standard free energy change will have a at 298 K.

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

Example: At 25°C, calculate the AG° N₂+ 3H2 → 2NH3 • AG° N2(g) = 0 kJ/mol f • AG + H2(g) = 0 kJ/mol f • AG˚ NH 3(g) = -16.66 kJ/mol f a) 12.9 kJ b) -33.3 kJ c) -16.7 kJ d) -8.33 kJ e) Unsure sys for: AG sys =ΣnpG˚ products - Σn,G° reactants 60
9
Km.201.
Aa.46. We start with a pure sample of A(g). The following equilibrium is established: 2 A(g) <---> B(g) + C(g) The total pressure is 8.75 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.20 atm. Calculate the value of the standard Gibbs free enthalphy change (in kJ) for this reaction at 25.0oC.
Gibbs free E 1
Given the below thermodynamic data, calculate ΔΔH for the reaction CH4 (g) + NH3 (g) ⟶⟶ HCN (g) + 3 H2 (g): N2 (g) + 3 H2 (g) ⟶⟶ 2 NH3 (g) ΔΔH = -85.6 kJ C (s) + 2 H2 (g) ⟶⟶ CH4 (g) ΔΔH = -75.2 kJ H2 (g) + 2 C (s) + N2 (g) ⟶⟶ 2 HCN (g) ΔΔH = +271.4 kJ
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) ⇒ 2NH₂(g) the standard change in Gibbs free energy is AG° = −32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH₂ = 0.750 atm? AG = 737 kJ/mol
Consider the Gibbs free energy change for the conversion of glucose to fructose that occurs during the metabolism of sugar (∆GRXN = +2.1 kJ) What is the value of the equilibrium constant (Keq) when the conversion takes place at 24.9 °C?
What is AGxn (in kJ) at 1932 K for the following reaction? 2POCI3(g) → 2PC13(g) + O₂(g) POCI3(g): AH = -592.7 kJ/mol and Sº = 324.6 J/K mol) PC13(g): AH = -287.0 kJ/mol and So = 311.7 J/K mol) O₂(g): AH = ? kJ/mol and Sº = 205.0 J/K mol)
Use the thermodynamic data provided below to determine the ΔGº for the reaction. 1A(s) + 4B(g) -> 1C(s) + 2D(g) Given the following: ΔGf° = -96.0 kJ mol-1 for substance A (s) ΔGfº = 254.0 kJ mol-1 for substance B (g) ΔGfº = 59.0 kJ mol-1 for substance C (s) ΔGfº= 248.0 kJ mol-1 for substance D (g) Provide your answer with final units of kJ and to one decimal place.
Mg(s) + 2 H2O(l) ⟶ Mg(OH)2(s) + 2H2(g) | ∆Hrxn = —353.0 kJ/mol Calculate the number of grams of Mg needed for this reaction to release enough energy to increase the temperature of 99 mL of water from 24 °C to 80. °C. Assume that the final mass of the solution is the same as the water, and that the density of solution is 0.997 g/mL. (10)
What is true about the following reaction at 25°C? H₂(g) + 2BrF(g) = 2HBr(g) + F₂(g) \Delta Hr\ deg = 115 kJ mol-¹ \Delta Sr\deg = 11.55 J mol-¹ K-¹ \Delta Gr\deg = 111 kJ mol-¹ i. The reaction is endothermic. ii. As the reaction proceeds heat is transferred from the surroundings to the system.