For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO(g) + 0,(g) =2 NO,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PNO = 0.500 atm, Po, = 0.350 atm, and PNO. = 0.800 atm?

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2 NO(g) + 0,(g) =2 NO,(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PNO = 0.500 atm, Po, = 0.350 atm, and PNO. = 0.800 atm?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 105QRT

See similar textbooks

Related questions

Q: At 25 ∘C, the equilibrium partial pressures for the reaction A(g)+2B(g)↽−−⇀C(g)+D(g) were found…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: When free energies (useful work) are estimated under standard conditions (1 atm pressure and 273.15…

Q: Calculate the standard change in Gibbs free energy, AGixn , for the given reaction at 25.0 °C.…

Q: Calculate the standard entropy, ASn, of the reaction at 25.0 °C using the table of thermodynamic…

A: From any reaction we can calculate the entropy change and Gibbs free energy change of the reaction .

Q: Suppose that in an industrial process N2 at 1.00 bar is mixed with H2 at 3.00 bar and the two gases…

Q: Consider the reaction: CaCO3(s) ↔ CaO(s) + CO2(g) The reaction enthalpy and entropy are: ΔHo rx =…

Q: Which of the following reactions will have the largest equilibrium constant (K) at 298 K? 1) 2…

A: The relationship between equilibrium constant (K) and standard free energy change (∆G°) is ∆G° = -…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

Q: The reaction C6H12O6 + 6O2 → 6CO2 + 6H2O ΔHo = −1072 kJ/mol and ΔSo =…

A: For the given reaction, ∆H° = -1072 kJ /mol = -1072 × 103 J mol-1 ∆S° = 578 J K-1 mol-1 T = 37 ℃ =…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

Q: Calculate the standard Gibbs free energy of the reaction, ΔG∘rxn. The standard enthalpy of the…

A: We have given that ∆G° of C2H4(g) = 68.4 KJ/mol ∆G° of H2O(l) = -237.1KJ/mol ∆G° of C2H5OH(l) =…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is 142. kJ.…

A: The free energy change of the reaction is = 142 kJ/mol The temperature of the reaction is = 5.00oC =…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction is -107. kJ. Calculate…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

Q: Determine AG° for the reaction 2 SO;(g) + 02(g) → 2 SO,(g) at 25 °C.

A: By this formula we can calculate the value of ∆G° for the given reaction . We have to put the given…

Q: For a certain chemical reaction, the standard Gibbs free energy of reaction at 5.00 °C is -76.7 kJ.…

Q: For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all…

A: According to the question, The standard Gibbs free energy is given by = ∆G° =-69.0 kJ/mol The…

Question

For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species.
For the reaction
2 NO(g) + 0,(g) =2 NO,(g)
the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial
pressures are PNO = 0.500 atm, Po,
= 0.350 atm, and PNO, = 0.800 atm?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2 Calculation

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).
Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy (H) for this reaction (assuming H is temperature-independent).
Silver carbonate, Ag2CO3, is a light yellow compound that decomposes when heated to give silver oxide and carbon dioxide: Ag2CO3(s)Ag2O(s)+CO2(g) A researcher measured the partial pressure of carbon dioxide over a sample of silver carbonate at 220C and found that it was 1.37 atm. Calculate the partial pressure of carbon dioxide at 25C. The standard enthalpies of formation of silver carbonate and silver oxide at 25C are 505.9 kJ/mol and 31.05 kJ/mol, respectively. Make any reasonable assumptions in your calculations. State the assumptions that you make, and note why you think they are reasonable.
One of the important reactions in the biochemical pathway glycolysis is the reaction of glucose-6-phosphate (G6P) to form fructose-6-phosphate (F6P): G6PF6PG298=1.7kJ (a) Is the reaction spontaneous or nonspontaneous under standard thermodynamic conditions?. (b) Standard thermodynamic conditions imply the concentrations of G6P and F6P to be 1 M, however, in a typical cell, they are not even Close to these values. Calculate G when the concentrations of G6P and F6P are 120 M and 28 M respectively, and discuss the spontaneity of the forward reaction under these conditions. Assume the temperature is 37 C.
Without looking up their standard entropies in reference tables, identify which of the following lists the materials in order of increasing entropy. (a) H2O() NaCl(s) NH3(g) (b) H2O() NH3(g) NaCl(s) (c) NaCl(s) H2O() NH3(g) (d) NH3(g) H2O() NaCl(s)
What is a spontaneous reaction?
Chemists and engineers who design nuclear power plants have to worry about high-temperature reactions because it is possible for water to decompose. (a) Under what conditions does this reaction occur spontaneously? 2H2O(g) 2H2(g) + O2(g) (b) Under conditions where the decomposition of water is spontaneous, do nuclear engineers have to worry about an oxygen/hydrogen explosion? Justify your answer.