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Fill in the blanks for the equilibrium of the reactants A+B with the products C+D. The temperature is 310K. When considering this table, it will be useful to know that the precision of the numbers provided is no better than ± 0.1 kJ/mole

Fill in the blanks for the equilibrium of the reactants A+B with the products C+D. The temperature is 310K. When considering this table, it will be useful to know that the precision of the numbers provided is no better than ± 0.1 kJ/mole

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Fill in the blanks for the equilibrium of the reactants A+B with the products C+D. The temperature is 310K. When considering this table, it will be useful to know that the precision of the numbers provided is no better than ± 0.1 kJ/mole.

 

 

### Thermodynamic Data Table This table provides information about the thermodynamics of a reaction involving four components: [A], [B], [C], and [D]. Each row represents a different condition with varying concentrations of these components. #### Column Descriptions: - **[A], [B], [C], [D]**: The concentrations of components A, B, C, and D, respectively. These are given in molarity (M) or millimolarity (mM, µM). - **ΔG°' (kJ mol⁻¹ K⁻¹)**: The standard Gibbs free energy change of the reaction. This value indicates whether the reaction is spontaneous under standard conditions. - **ΔG' (kJ mol⁻¹ K⁻¹)**: The Gibbs free energy change under the specific conditions of the row. This value can differ from ΔG°' due to the non-standard concentrations of reactants and products. - **At Equilibrium?**: Indicates whether the reaction is at equilibrium under the given conditions. A reaction at equilibrium will not show net change in the concentrations of reactants and products over time. - **Direction Favorable?**: Indicates if the reaction is thermodynamically favorable in the forward direction under the given conditions. #### Row Descriptions: 1. **Row 1**: - [A], [B], [C], [D] = 1 M, 1 M, 1 M, 1 M - ΔG°' = -20.0 kJ mol⁻¹ K⁻¹, ΔG' = -20.0 kJ mol⁻¹ K⁻¹ - At Equilibrium: No - Direction Favorable: Yes 2. **Row 2**: - [A], [B], [C], [D] = 2 mM, 1 mM, 0.0135 M, 50 mM - ΔG°' = ?, ΔG' = 30.0 kJ mol⁻¹ K⁻¹ - At Equilibrium: No - Direction Favorable: No 3. **Row 3**: - [A], [B], [C], [D] = 2 mM, 1 mM, 0.001 M, 50 mM - Δ
Transcribed Image Text:### Thermodynamic Data Table This table provides information about the thermodynamics of a reaction involving four components: [A], [B], [C], and [D]. Each row represents a different condition with varying concentrations of these components. #### Column Descriptions: - **[A], [B], [C], [D]**: The concentrations of components A, B, C, and D, respectively. These are given in molarity (M) or millimolarity (mM, µM). - **ΔG°' (kJ mol⁻¹ K⁻¹)**: The standard Gibbs free energy change of the reaction. This value indicates whether the reaction is spontaneous under standard conditions. - **ΔG' (kJ mol⁻¹ K⁻¹)**: The Gibbs free energy change under the specific conditions of the row. This value can differ from ΔG°' due to the non-standard concentrations of reactants and products. - **At Equilibrium?**: Indicates whether the reaction is at equilibrium under the given conditions. A reaction at equilibrium will not show net change in the concentrations of reactants and products over time. - **Direction Favorable?**: Indicates if the reaction is thermodynamically favorable in the forward direction under the given conditions. #### Row Descriptions: 1. **Row 1**: - [A], [B], [C], [D] = 1 M, 1 M, 1 M, 1 M - ΔG°' = -20.0 kJ mol⁻¹ K⁻¹, ΔG' = -20.0 kJ mol⁻¹ K⁻¹ - At Equilibrium: No - Direction Favorable: Yes 2. **Row 2**: - [A], [B], [C], [D] = 2 mM, 1 mM, 0.0135 M, 50 mM - ΔG°' = ?, ΔG' = 30.0 kJ mol⁻¹ K⁻¹ - At Equilibrium: No - Direction Favorable: No 3. **Row 3**: - [A], [B], [C], [D] = 2 mM, 1 mM, 0.001 M, 50 mM - Δ
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