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calculated from of formation of the substances involved in the reaction: AHxn=AH (products) - AH (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AG. The Gibbs free energy depends on both the enthalpy and entropy changes. ▼ Hint 1. How to approach the problem In the previous part, you determined that the enthalpy AHxn was 229 kJ for the reaction written. This means that 229 kJ of heat is absorbed when exactly 2 mol of A and 1 mol of react to produce 2 mol of C and 2 mol of D according to the balanced chemical equation 2A + B 2C+ 2D When less A reacts, less heat is absorbed. When more A reacts, more heat is absorbed. S up the heat absorbed to correspond to 2.60 mol of A.

calculated from of formation of the substances involved in the reaction: AHxn=AH (products) - AH (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AG. The Gibbs free energy depends on both the enthalpy and entropy changes. ▼ Hint 1. How to approach the problem In the previous part, you determined that the enthalpy AHxn was 229 kJ for the reaction written. This means that 229 kJ of heat is absorbed when exactly 2 mol of A and 1 mol of react to produce 2 mol of C and 2 mol of D according to the balanced chemical equation 2A + B 2C+ 2D When less A reacts, less heat is absorbed. When more A reacts, more heat is absorbed. S up the heat absorbed to correspond to 2.60 mol of A.

Chemistry
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
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Part b For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? And part c said At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH (products) - AH (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: ΔG° = ΔΗ° -ΤΔS where T is standard temperature, 298 K. Part B For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? Express your answer numerically in kilojoules. ▾ View Available Hint(s) ▼ ▼ Review | Constants | Periodic Table Hint 1. How to approach the problem In the previous part, you determined that the enthalpy AH was 229 kJ for the reaction as written. This means that 229 kJ of heat is absorbed when exactly 2 mol of A and 1 mol of B react to produce 2 mol of C and 2 mol of D according to the balanced chemical equation 2A + B 2C + 2D When less A reacts, less heat is absorbed. When more A reacts, more heat is absorbed. Scale up the heat absorbed to correspond to 2.60 mol of A. Hint 2. Determine the heat absorbed per mole of A Given the enthalpy of this reaction as written 2A + B 2C + 2D, how much heat is absorbed for each mole of A that reacts? AHxn = 229kJ
Transcribed Image Text:Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH (products) - AH (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: ΔG° = ΔΗ° -ΤΔS where T is standard temperature, 298 K. Part B For the reaction given in Part A, how much heat is absorbed when 2.60 mol of A reacts? Express your answer numerically in kilojoules. ▾ View Available Hint(s) ▼ ▼ Review | Constants | Periodic Table Hint 1. How to approach the problem In the previous part, you determined that the enthalpy AH was 229 kJ for the reaction as written. This means that 229 kJ of heat is absorbed when exactly 2 mol of A and 1 mol of B react to produce 2 mol of C and 2 mol of D according to the balanced chemical equation 2A + B 2C + 2D When less A reacts, less heat is absorbed. When more A reacts, more heat is absorbed. Scale up the heat absorbed to correspond to 2.60 mol of A. Hint 2. Determine the heat absorbed per mole of A Given the enthalpy of this reaction as written 2A + B 2C + 2D, how much heat is absorbed for each mole of A that reacts? AHxn = 229kJ
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH; (products) - AH; (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH - TAS° where I is standard temperature, 298 K. ▼ Part C For the reaction given in Part A, ASn is 23.0 J/K. What is the standard Gibbs free energy of the reaction, AG? Express your answer numerically in kilojoules. ▾ View Available Hint(s) Hint 1. How to approach the problem Start by converting the enthalpy change to joules.Then use the equation AG=AH° - TAS symbol means "standard." Standard temperature in In quantities such as AG, the thermodynamics is 298 K. Hint 2. Convert the enthalpy to match the units of entropy
Transcribed Image Text:Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH; (products) - AH; (reactants) Entropy change, AS, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH - TAS° where I is standard temperature, 298 K. ▼ Part C For the reaction given in Part A, ASn is 23.0 J/K. What is the standard Gibbs free energy of the reaction, AG? Express your answer numerically in kilojoules. ▾ View Available Hint(s) Hint 1. How to approach the problem Start by converting the enthalpy change to joules.Then use the equation AG=AH° - TAS symbol means "standard." Standard temperature in In quantities such as AG, the thermodynamics is 298 K. Hint 2. Convert the enthalpy to match the units of entropy
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