Answered: at 25 ̊C , calculate the ΔG ̊sys for:…

at 25 ̊C , calculate the ΔG ̊sys for: N2 + 3H2 → 2NH3 ΔG ̊f N2(g) = 0 kJ/mol ΔG ̊f H2(g) = 0 kJ/mol ΔG ̊f NH3(g) = -16.66 kJ/mola) 12.9 kJb) -33.3 kJc) -16.7 kJd) -8.33 kJe) Unsure

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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choose the right options -When a solid dissolves in a liquid, entropy usually (increases or decreases?) So the value for ΔΔS is (positive or negative?) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, solids are usually more soluble at (higher or lower?) temperatures. When a gas dissolves in a liquid, entropy usually (increases or decreases), so the value for ΔΔS is (negative or postive) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, gases are usually more soluble at (lower or higher) temperatures.
Calculate ΔG for the reaction below, where the T = 298K, ΔH = 28.05 kJ, and the ΔS = 109 J/K. NH4NO3(s) + H2O(l) NH4+ (aq) + NO3- (aq)
Calculate ΔG in kJ•mol-1 at 298 K for the following reaction: 2 A(g) + B2(s) → 2 AB(g) ΔGo = 49 kJ•mol-1 under the following conditions: P(A) = 0.446 atm, P(AB) = 0.823 atm A certain reaction A → B has a rate constant of 4.7 x 10–2 M s-1 at 25°C. An experiment was run at this temperature where the initial concentration of A is 0.342 M. What is the half-life of the reaction in seconds? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)
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.
What is the reaction that represents ΔHf° for Al2O3 (s)?
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
Calculate delta G for the reaction, 2A (g) + B2(g) —- 2AB(g) given that at 120 C the equilibrium constant of the reaction is 3.12 x 10^5 -41.43 j/mol -41.43 kj/mol None of the above -35.76 kj/mol -414.30 j/mol