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In the reaction shown below, the standard Gibbs energy of formation and standard enthalpy of formation of the reactants and products at 25°C are given. Calculate the standard Gibbs energy of reaction, the standard enthalpy (kJ/mol) of reaction, and the equilibrium constant at 298K. A 4G (KJmol-1) -160.55 AH (KJmol-1) -178.12 (a) 4.G°(298K)= (b)4 H°(298K)= (c)K(298K)= + B -167.17 -141.53 = C + D -31.22 -79.55 -344.36 -393.51 (kJ/mol, round to 2 decimals, such as -25.67) (kJ/mol, round to 2 decimals, such as -25.67) (use E notation with 1 decimal such as 2.5E3 for 2515)

In the reaction shown below, the standard Gibbs energy of formation and standard enthalpy of formation of the reactants and products at 25°C are given. Calculate the standard Gibbs energy of reaction, the standard enthalpy (kJ/mol) of reaction, and the equilibrium constant at 298K. A 4G (KJmol-1) -160.55 AH (KJmol-1) -178.12 (a) 4.G°(298K)= (b)4 H°(298K)= (c)K(298K)= + B -167.17 -141.53 = C + D -31.22 -79.55 -344.36 -393.51 (kJ/mol, round to 2 decimals, such as -25.67) (kJ/mol, round to 2 decimals, such as -25.67) (use E notation with 1 decimal such as 2.5E3 for 2515)

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
Section: Chapter Questions
Problem 83QRT: Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate,...
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plz answer 5 and i use 6 for a follow up question

QUESTION 5 In the reaction shown below, the standard Gibbs energy of formation and standard enthalpy of formation of the reactants and products at 25°C are given. Calculate the standard Gibbs energy of reaction, the standard enthalpy (kJ/mol) of reaction, and the equilibrium constant at 298K. A 4G (KJmol-1) 4H°(KJmol-1) (a) 4,Gᵒ(298K)= (b)4 H°(298K)= (c)K(298K)= -160.55 -178.12 + B -167.17 = C + D -141.53 -31.22 -344.36 -79.55 -393.51 (kJ/mol, round to 2 decimals, such as -25.67) (kJ/mol, round to 2 decimals, such as -25.67) (use E notation with 1 decimal such as 2.5E3 for 2515) QUESTION 6 Continue with the last question, based on your calculated AH°, is the reaction endothermic or exothemic? According to Le Chatelier's principle which direction will the reaction shift to if temperature is raised? O The reaction is endothermic, and the reaction shifts towards reactants when temperature is raised. O The reaction is exothermic, and the reaction shifts towards products when temperature is raised. O The reaction is exothermic, and the reaction shifts towards reactants when temperature is raised. O The reaction is endothermic, and the reaction shifts towards products when temperature is raised.
Transcribed Image Text:QUESTION 5 In the reaction shown below, the standard Gibbs energy of formation and standard enthalpy of formation of the reactants and products at 25°C are given. Calculate the standard Gibbs energy of reaction, the standard enthalpy (kJ/mol) of reaction, and the equilibrium constant at 298K. A 4G (KJmol-1) 4H°(KJmol-1) (a) 4,Gᵒ(298K)= (b)4 H°(298K)= (c)K(298K)= -160.55 -178.12 + B -167.17 = C + D -141.53 -31.22 -344.36 -79.55 -393.51 (kJ/mol, round to 2 decimals, such as -25.67) (kJ/mol, round to 2 decimals, such as -25.67) (use E notation with 1 decimal such as 2.5E3 for 2515) QUESTION 6 Continue with the last question, based on your calculated AH°, is the reaction endothermic or exothemic? According to Le Chatelier's principle which direction will the reaction shift to if temperature is raised? O The reaction is endothermic, and the reaction shifts towards reactants when temperature is raised. O The reaction is exothermic, and the reaction shifts towards products when temperature is raised. O The reaction is exothermic, and the reaction shifts towards reactants when temperature is raised. O The reaction is endothermic, and the reaction shifts towards products when temperature is raised.
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