Calculate Δ G ∘ rxn for the following reaction: 4CO(g)+2N O 2(g)→4C O 2 (g)+ N 2 (g) . Use the following reactions and given Δ G∘ rxn values: 2NO(g)+ O 2 (g)→2N O 2 (g) , Δ G ∘ rxn = - 72.6 kJ2CO(g)+ O 2 (g)→2C O 2 (g) , Δ G ∘ rxn = - 514.4 kJ 1 2 O 2 (g)+ 12 N 2 (g)→NO(g) , Δ G ∘ rxn = 87.6 kJ Express your answer using onedecimal place. Δ G ∘ rxn = nothing kJ 2) Consider the followingreaction:
CO(g)+2H2(g)⇌CH3OH(g)
Kp=2.26×104 at 25 ∘C. Calculate ΔGrxn for thereaction at 25 ∘C under each of the following conditions.​  

Part A

standard conditions

ΔGrxn =		kJ

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Part B

at equilibrium

ΔGrxn =		kJ

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Part C

PCH3OH= 1.1 atm ;
PCO=PH2= 1.5×10^−2 atm

Express your answer using two significant figures.

3)

For the decomposition of barium carbonate, considerthe following thermodynamic data (Due to variations inthermodynamic values for different sources, be sure to use thegiven values in calculating your answer.): ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the temperature in kelvins above which this reaction isspontaneous. Express your answer to four significant figures and include theappropriate units. View Available Hint(s) SubmitPrevious AnswersRequest Answer Relationship between free energy and the equilibriumconstant The standard free energy change, ΔG∘ , and the equilibriumconstant K for a reaction can be related by the followingequation: ΔG∘=−RTlnK where T is the Kelvin temperature and R is equalto 8.314 J/(mol⋅K) . Part B Part complete The thermodynamic values from part A will be useful as you workthrough part B: T = nothing nothing ΔH∘rxn 243.5kJ/mol ΔS∘rxn 172.0J/(mol⋅K) Calculate the equilibrium constant for the following reaction atroom temperature, 25 ∘C : BaCO3(s)→BaO(s)+CO2(g) K = nothing