At 25°C, calculate the AG, N₂+ 3H2 → 2NH3 sys for: f • AG˚ N2(g) = 0 kJ/mol AG H2(g) = 0 kJ/mol f • AG˚ NH3(g) = -16.66 kJ/mol f a) 12.9 kJ b) -33.3 kJ c) -16.7 kJ d) -8.33 kJ e) Unsure AG sys =ΣnpG˚ products - Σn,G° reactants 60

A)Consider these hypothetical chemical reactions: A⇌B,ΔG=A⇌B,ΔG= 13.5 kJ/molkJ/mol B⇌C,ΔG=B⇌C,ΔG= -27.6 kJ/molkJ/mol C⇌D,ΔG=C⇌D,ΔG= 9.90 kJ/molkJ/mol What is the free energy, ΔGΔGDelta G, for the overall reaction, A⇌DA⇌D?   B)Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions are: luciferin+O2ATP⇌oxyluciferin+light ATP⇌AMP+PPi If the overall ΔGDelta G of the coupled reaction is -9.00 kJ/mol , what is the equilibrium constant, KKK, of the first reactions at 13 ∘C ? The ΔGDelta for the hydrolysis of ATP to AMP is −31.6 kJ/mol. Express your answer numerically.

Using the equation, ΔG=ΔH−TΔS, explain when will ΔG<0, ΔG>0 and ΔG=0

Consider 8 the following reaction: 2NH3(g) + CO2(g) → NH2CONH2(aq) + H2O(l) ∆G° = -13.6 kJ at 25°C What is the value of ∆G at 25°C for this reaction under the following set of conditions? 25.0 atm NH3 (g) 0.500 atm CO2 (g) 1.00 M NH2CONH2 (aq) Group of answer choices -18.1 kJ 0.63 kJ -27.8 kJ 14.2 kJ -20.0 kJ

Given the following data, what is the value of ΔGf° (CH3OH(ℓ) at 25°C?CO(g) + 2 H2(g) ⇄ CH3OH(ℓ)   K = 1.081 × 10-40ΔGf°(CO) = -137.2 kJ/mol

What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 5.95e-5?5C2H2(g) + 6 H2(g) → C10H22(g) ΔGo = -1.01e3 kJ. a) ΔG = -1.036e3 kJ b) ΔG = -1.010e3 kJ c) ΔG = -1.014e3 kJ d) ΔG = 1.057e3 kJ

a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) =  -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l)  b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?

Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of the reactants and products.Compound ΔGof (kJmol)ΔGfo(kJmol)    The equation H2O(l) → H2O(g)  ΔGoΔGokJ C2H2(g)209.9 CO2(g)-394.4 H2O(g)-228.6 H2O(l)-237.1 N2(g)0 NO(g)87.6 O2(g)0

) Calculate the ΔG°rxn using the following information.                     4 HNO3(g) + 5 N2H4(l) → 7 N2(g) + 12 H2O(l)       ΔG°rxn = ? ΔG°f (kJ/mol) -73.5          149.3                          -237.1

One of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate ΔG° (at 298 K) for this reaction. AG = -198 kJ b Calculate K (at 298 K) for this reaction. K =