The difference in chemical potential of a particular substance between two regions of a system is +7.1 kJ mol−1. By how much does the Gibbs energy change when 0.10 mmol of that substance is transferred from one region to the other?

The difference in chemical potential of a particular substance between two regions of a system is +7.1 kJ mol−1. By how much does the Gibbs energy change when 0.10 mmol of that substance is transferred from one region to the other?

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 91QRT: Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium...

See similar textbooks

Related questions

Q: Question attached

A: The change in Gibbs free energy = -2808 kJ mol-1 Mass of the person = 65 kg

Q: Ethylene glycol is a common ingredient in antifreeze. It has a molar mass of 62.068 g mol-1 and a…

A: Please find your solution below : Gibbs free energy is a thermodynamic quantity which is used to…

Q: Estimate the change in the Gibbs energy and molar Gibbs energy of 100 cm3 of water when the pressure…

Q: Calculate the standard Gibbs energy of the reaction CO(g) + CH3CH2OH(l) → CH3CH2COOH(l) at 298 K,…

A: The given reaction is shown below. The value of ΔH°f(CO)=-110.525 kJ/mol ΔS°m (CO)=197.674 J/Kmol…

Q: The standard state of a substance used to be defined as 1 atm at the specified temperature. By how…

A: Given data:

Q: Calculate the standard molar Gibbs energy of neon gas at 298 K.

A: The standard molar Gibbs energy at any temperature T can be expressed as follows:

Q: The decomposition of a generic diatomic element in its standard state is represented by the equation…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: b. The standard enthalpy of formation of gaseous NH3 at 298 K is -46.11 kJmor'. Estimate che…

Q: Calculate the standard reaction entropy at 298 K when 1 mol NH3(g) is formed from its elements in…

A: Given: Temperature(T)= 298 K When 1 mol of NH3 is formed from its elements in their reference…

Q: Calculate the standard reaction entropy and the standard Gibbs energy at 298 K of reaction…

Q: The change in the Gibbs energy of a certain constant-pressure process is found to fit the expression…

A: The given equation is, The relation between free energy, enthalpy and entropy is given by the…

Q: The difference in chemical potential between two regions of a system is -8.3 kJ mo1. By how much…

A: The given data contains, difference in chemical potential =-8.3 KJ/mol dn =0.15 mmol

Q: C. Consider a chemical reaction. At a temperature T, = 300. K and an external pressure P, the…

A: In question you have to ask particularly to find the value of ∆r G(T2,P) Gibbs free energy at T2 =…

Q: What proportions of hexane and heptane should be mixed (i) by mole fraction, (ii) by mass in order…

Q: The decomposition of a generic diatomic element in its standard state is represented by the equation…

A: The following formula is applied to solve for the answer. ∆G°=-RTln(K') where, '∆G°' is the standard…

Q: The difference in a chemical potential of a particular substance between two regions of a system is…

A: The Gibbs energy change for transfer of dn moles of a substance from region 1 with chemical…

Q: For a certain constant-pressure process, the change in Gibbs energy was found to fit the expression:…

A: Since for any process, the relationship between G, H and S is given by G = H - TS The expression…

Q: The standard Gibbs energy of the reaction N2(g) + 3 H2(g) → 2 NH3(g) is −32.9 kJ mol−1 at 298 K.…

Q: The standard molar entropies of water ice, liquid, and vapour at 298 K are 37.99, 69.91, and 188.83…

A: Given, The standard molar entropies of water ice, liquid, and vapour at 298 K are 37.99, 69.91 and…

Q: Calculate the difference in Gibbs energy of a perfect gas if the pressure is increased by 20% at…

A: Gibbs free Energy (ΔG): In a reversible system at constant temperature and pressure, Gibbs energy is…

Q: When the reaction 2 A → B advances by 0.051 mol (i.e. Δξ = +0.051 mol) the molar Gibbs energy of the…

A: Gibbs free energy of a reaction is the maximum energy or work that can be obtained from any…

Q: The difference in a chemical potential of a particular substance between two regions of a system is…

A: Change in mole = 0.15 mmol Change in chemical potential = - 8.3 kJ/mol

Q: The Gibbs energy of a pure substance is identical to another thermodynamic quantity: the chemical…

A: Hello. Since the question contains multiple parts, the first part is solved. In case the solution…

Q: 8) The changes in Gibbs energy of a certain constant pressure process is found to fit the expression…

Q: Estimate the change in the Gibbs energy of 100cm3 of water when the pressure acting on it is…

A: Volume of water = 100cm^3 Initial pressure = 100kPa Final Pressure = 500kPa Mass density of water =…

Q: If we have a hydrophobic molecule in aqueous solution that makes contact with 25 water molecules,…

A: Hydrophobic molecules do not interact with the water molecule at normal temperature. Mixing of…

Q: The standard reaction Gibbs energy of the isomerization of borneol (C10H17OH) to isoborneol in the…

A: Given: ΔGo = 9.4 KJ/mol = 9400 J/mol. Moles of borneol = 0.15 mol. Moles of isoborneol = 0.30 mol.…

Q: Calculate the standard reaction entropy at 298 K when 1 mol N2O(g) is formed from its elements in…

A: The involved chemical equation would be: N2 (g) + ½ O2 (g) → N2O (g)

Q: The chemical potential of a particular substance in the region A of a system is 5kJ higher than…

A: Since the relationship between change in gibbs free energy and chemical potential is given by ΔG =…

Q: Question attached

A: The equation relating Gibb's free energy(∆G) and enthalpy (∆H) is; ∆G=∆H-T∆ST=Temperature∆S=change…

Q: The standard Gibbs energy of formation of rhombic sulfur is zero and that of monoclinic sulfur is…

A: In this question, we will see which polymorph is most stable at 25°V temperature. You can see…

Q: The equilibrium constant associated with the gas phase reaction between SO2 and oxygen forming SO3…

Q: Calculate the change in molar Gibbs energy of carbon dioxide (treated as a perfect gas) at 20 °c…

A: Gibbs free energy is a thermodynamic quantity ∆G: Molar Gibbs energy can be calculated by using the…

Q: The change in the Gibbs energy of a certain constant-pressure process was found to fit the…

Q: The decomposition of a generic diatomic element in its standard state is represented by the equation…

Q: Calculate the change in the molar Gibbs energy of nitrogen gas when its pressure is increased…

A: We have given that Temperature (T) = 298 K Initial pressure (Pi) = 1 atm Final pressure (Pf) = 50…

Q: C. Consider a chemical reaction. At a temperature T1 enthalpy of reaction is A,H(T,, P) = 400. J and…

A: By studying the temperature, enthalpy, and Gibbs free energy we can conclude that if the reaction is…

Q: 9) Estimate the change in the Gibbs energy of 100 cm³ of water when the pressure acting on it is…

A: Gibbs free energy is also known as free energy: It is defined as the measure of the maximum…

Q: The change in the Gibbs energy of a certain constant-pressure process was found to fit the…

A: Given , The process is constant pressure process.

Q: Estimate the change in the Gibbs energy of 100 cm3 of water when the pressure acting on it is…

A: Change in Gibb's energy: This is the energy that is used from the initial stage to the final stage…

Q: Use the fundamental equation of therodynamics here to calculate the change Gibbs energy when 3.1…

A: The change in free energy (∆G) is expressed as ∆G = ∆H = T∆S where ∆H is the change in enthalpy, ∆S…

Q: The standard molar entropy of benzene is 173.3 J K-1 mol-1. Calculate the change in its standard…

A: The given data contains, Standard molar entropy of benzene= 173.3 J/K.mol Temperature T1= 25°C=298 K…

Q: Estimate the change in the Gibbs energy of 1.0 dm3 of liquid octane when the pressure acting on it…

A: Given:VolumeV=1.0dm3 Initial pressureP1=1.0atmFinal pressureP2=100atmMass density of octane=0.703g…

Q: The standard reaction Gibbs energy of the isomerization of borneol (C10H17OH) to isoborneol in the…

A: Given: Standard Gibbs energy (ΔGo) = +94 KJ/mol Temperature (T) = 503 K Total pressure Ptotal = 600…

Q: The change in Gibbs energy that accompanies the combustion of C6H12O6(s) to carbon dioxide and water…

A: The given data contains, change in Gibbs free energy = -2828 kj/mol mass of person= 65 kg

Q: a. Calculate the standard Gibbs free energy change for the process of dissolution of benzene in…

A: Gibbs free energy(∆G) The decrease in the value of Gibbs free energy during a process is equal…

Q: Calculate the change in the molar Gibbs energy of a perfect gas when its pressure is increased…

A: Given that: Pressure (P1) = 1.0 atm Pressure (P2) = 100.0 atm Temperature (T) = 298 K Change in…

Question

The difference in chemical potential of a particular substance between two regions of a system is +7.1 kJ mol⁻¹. By how much does the Gibbs energy change when 0.10 mmol of that substance is transferred from one region to the other?

Expert Solution

This question has been solved!

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

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

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

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.
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().
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?)
Consider planet Earth as a thermodynamic system. Is Earth thermodynamically or kinetically stable? Discuss your choice, providing as many arguments as you can tosupport it.
Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.
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)
The decomposition of a generic diatomic element in its standard state is represented by the equation 1/2 X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.58 kJ·mol−1 at 2000 K and −52.64 kJ·mol−1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, ?K, at each temperature. At 2000 K, ΔGf=5.58 kJ·mol−1. What is ? at that temperature? At 3000 K, Δ?f=−52.64 kJ·mol−1. What is K at that temperature?
The decomposition of a generic diatomic element in its standard state is represented by the equation 1/2 X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.34 kJ·mol−1 at 2000. K and−50.82 kJ·mol−1 at 30003000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, ΔGf=4.34 kJ·mol−1. What is K at that temperature?
Hydrogen gas burns in an atmosphere of bromine gas to produce hydrogen bromide gas according to the chemical reaction H, (g) + Br, (g) → 2 HBr(g) Calculate the standard Gibbs free energy of the reaction. Refer to the list of thermodynamic values. AGixn = kJ-mol-! Suppose 130.0 mL of hydrogen gas at STP combines with a stoichiometric amount of bromine gas and the resulting hydrogen bromide dissolves in water to form 185.0 mL of an aqueous solution. What is the concentration of the resulting hydrobromic acid? concentration: M
The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =
he decomposition of a generic diatomic element in its standard state is represented by the equation 12X2(g)⟶X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.20 kJ·mol−1 at 2000. K and −53.38 kJ·mol−1 at 3000. K. Determine the value of the thermodynamic equilibrium constant, ?, at each temperature. At 2000. K, Δ?f=4.20 kJ·mol−1. What is ? at that temperature? ? at 2000. K= At 3000. K, Δ?f=−53.38 kJ·mol−1. What is K at that temperature? ? at 3000. K=
If the equilibrium constant of a reaction is Keq = 9.3 × 103 at 900 °C, what is the change in Gibbs free energy for this reaction (in kJ mol–1) at the indicated temperature? R = 8.314 J K–1 mol–1