b. The standard enthalpy of formation of gaseous NH3 at 298 K is -46.11 kJmor'. Estimate che standard enthalpy of formation of gaseous NH3 at 400 K given that the molar heat capacities of NH3(g),H2(g)and N2(g)are 36.0,28.2 and 29.1J K' mor,respectively. If the standard Gibbs energy of formation of NH3(g) at 298 K is -16.45 kJ mor1 estimate the standard Gibbs energy of formation at 400 K.

b. The standard enthalpy of formation of gaseous NH3 at 298 K is -46.11 kJmor'. Estimate che standard enthalpy of formation of gaseous NH3 at 400 K given that the molar heat capacities of NH3(g),H2(g)and N2(g)are 36.0,28.2 and 29.1J K' mor,respectively. If the standard Gibbs energy of formation of NH3(g) at 298 K is -16.45 kJ mor1 estimate the standard Gibbs energy of formation at 400 K.

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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(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. ____The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -).____A Gibbs free energy change involves moles of substances whereas an emf involves coulombs of electrons.____A coulomb of particles is more particles than a mole of particles.____Faraday's constant is not used to interconvert a Gibbs free energy change and a reaction emf.____A Gibbs free energy change involves coulombs of substances whereas an emf involves moles of electrons.Calculate the standard Gibbs free energy changes at 25 oC for each of the reactions shown below using the Eo values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 1 Al3+(aq) + 3 Ag(s) 1 Al(s) + 3 Ag+(aq) Eo = -2.459 V Go =________ kJ/mol ____nonspontaneous…
MISSED THIS? Read Section 19.8 (Pages 871-877); Watch IWE 19.6. Liquid methanol burns in oxygen to form gaseous carbon dioxide and gaseous water. Substance H (kJ/mol) S° (J/(mol · K)) CH, OH (1) -238.6 126.8 O₂(g) 0 205.2 CO₂(g) -393.5 213.8 CO2(aq) -413.8 117.6 H₂O(g) -241.8 188.8 H₂O(1) -187.8 70.0 ▼ Part D where no represents the stoichiometric coefficients of the products, n, represents the st of the reactants, and Sº represents the standard entropies. AGxn= Calculate AG at 25°C. Express your answer in kilojoules to three significant figures. Submit = Provide Feedback 15] ΑΣΦ Request Answer Part E Complete previous part(s) [2(S° co₂(g)) + 4(S° H₂O(g))]- [2(S° CH₂OH()) + 3(S° 0₂(E [2(213.8 J/K)+4(188.8 J/K)] - [2(126.8 J/K) + 3(2 314 J/K MacBook Pro P Pearson ? kJ Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions Contac
A reaction, run at 298 Kand constant pressure, is found to have a standard Gibbs free energy of –181.6 K. If standard change in entropy for the reaction is found to be mole -165.2 k how much heat (in kJ) was released in the reaction? mole Type your answer.
3. Use the appropriate data from the table to calculate the change in enthalpy for this reaction: Mg) + 2HClag) > M9CI2(ag) + H2(9) (aq) Species AH", , kJ/1mol HCl(g) -92.30 HCl(aq) -167.2 MgCl(s) -641.6 MgCla(aq) -796.9 H,O(1) -285.83 4. Using your answer for question #3, how much energy would be produced from the reaction of 0.680g of Mg with excess hydrochloric acid?
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Half a mole of a perfect gas expands isothermally and at 298.15 K from a volume of 10 L to avolume of 20 L. (a) What is the change in the entropy of the gas? (b) How much work is doneon the gas? (c) What is the heat of Surroundings ? (d) What is the change in the entropy of the surroundings? (e)What is the change in the entropy of the system plus the surroundings?
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