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)
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Publisher:John W. Moore, Conrad L. Stanitski
Chapter16: Thermodynamics: Directionality Of Chemical Reactions
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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F63f5865a-7713-44c4-be73-1c5678c4385b%2Fbf16eb26-90ff-4ad5-8c2c-780ce86f9c6c%2F2gqs087_processed.jpeg&w=3840&q=75)
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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