Make a non-spontaneous process spontaneousA process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous.The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highlyspontaneous:C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1)Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropyto argue this reaction is highly spontaneous? Gibbs free energy (G) is a measure of thespontaneity of a chemical reaction. It is thechemical potential for a reaction, and is minimizedat equilibrium. It is defined asG=H-TSwhere H is enthalpy, T is temperature, and S isentropy.The chemical reaction that causes magnesium tocorrode in air is given by2Mg + O2-2MgOin which at 298 K, AHASixm 217.1 J/K.== - 1204 kJ and=Part AWhat is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of298 K.Express your answer as an integer and include the appropriate units.► View Available Hint(s)AGrxn =μÅValueUnits?

A reaction at the given condition that results in the favorable formation of products is called a…

Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes magnesium to corrode in air is given by 2Mg + O2-2MgO in which at 298 K, AH = 1204 kJ and AS = - 217.1 J/K. - ▼ Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) AGixn= O μA Value Units ?

Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes magnesium to corrode in air is given by 2Mg + O2-2MgO in which at 298 K, AH = 1204 kJ and AS = - 217.1 J/K. - ▼ Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ► View Available Hint(s) AGixn= O μA Value Units ?

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...

See similar textbooks

Similar questions

The second law of thermodynamics states that for a process to be spontaneous: (A) The entropy of the system must increase; (B) The energy of the system must decrease; (C) The energy of the universe must decrease. (D) The entropy of the universe must increase;
What is the maximum work that could be obtained (in kJ) from 4.85 g of zinc metal in the following reaction at 25°C? Zn(s) + Cu2+(aq) --> Zn2+(aq) + Cu(s) Give your answer numerically, assuming a measure of kJ
For the reaction Ca(OH)2 (aq) + 2HCl(aq) → CaCl₂ (s) + 2H₂O(1) = 206 J/K The equilibrium constant for this reaction at 341.0 K is Assume that AH° and ASº are independent of temperature. ΔΗ° = -30.2 kJ and AS⁰
At 125 °C, 1 mol O2 and 2 mol H₂ in a chamber have a total pressure of 3 atm. A current is run through the chamber, combining all the molecules into H₂O at constant volume. The pressure of the chamber, in atmospheres, is now:
Calculate the standard Gibbs free energy for the following reaction at 25 °C and 1 atm. Based on your calculations, predict whether the reaction will occur spontaneously or not. H2O (l) → H2 (g) + ½ O2 (g). Calculate ΔG° using the two different methods we covered in class. (answer for both methods = +237 kJ/mol)
The industrial synthesis of chloroform by the reaction of methane with Cl2 is carried out according to the following reaction equation:CH4 (g) + Cl2 (g) → CHCl3 (l) + HCl (g)Using the thermodynamic data provided, calculate Ho (in Kj/mol) for this reaction.
A chemist measures the enthalpy change AH during the following reaction: 2H,0(1) + O,(g)→2H,O2(1) AH=196. kJ Use this information to complete the table below. Round each of your answers to the nearest kJ/mo reaction ΔΗ x10 6H,0,(1) → 6H,0(1) + 30,(g) 4H,0(1) + 20,(g) → 4H,0,(1) I kJ 2H,0,(1) → 2H,0(1) + 0,(g) kJ
Do
Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T' is temperature, and S is entropy. The chemical reaction that causes aluminum to corrode in air is given by 4A1+30₂-2Al₂O₁ in which at 298 K, AH = -3352 kJ and AS = -625.1J/K Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K Express your answer as an integer and include the appropriate units. ▸ View Available Hint(s) μA AG - 89 kJ Submit Previous Answers X Incorrect; Try Again; 4 attempts remaining Part B What is the Gibbs free energy for this reaction at 5975 K? Assume that AH and AS do not change with temperature. Express your answer to two decimal places and include the appropriate units. > View Available Hint(s) ? AG= Value Units Submit
Calculate the standard enthalpy change for the reaction at 25 °C. Standard enthalpy of formation values can be found in this list of thermodynamic properties. C,H,() +50,(g) – 3CO,(g) + 4 H,O(g) kJ AHan =
Write the chemical equation for the standard molar enthalpy of formation of nitromethane, CH3NO2.
Calculate Ecell and E0Cell along with delta G and the equilibrium constant