plz answer 5 and i use 6 for a follow up question QUESTION 5In the reaction shown below, the standard Gibbs energy of formation and standard enthalpy of formation of the reactants andproducts at 25°C are given. Calculate the standard Gibbs energy of reaction, the standard enthalpy (kJ/mol) of reaction, and theequilibrium constant at 298K.A4G (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 6Continue with the last question, based on your calculated AH°, is the reaction endothermic or exothemic? According to LeChatelier'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.

Given reaction is A + B ⇔ C + D Standard Gibbs energy of reaction is given by the formula, ∆rGo…

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

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...

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