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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The potassium-ion concentration in blood plasma is about 5.0 * 10-3 M, whereas the concentration in muscle-cell fluid is much greater (0.15 M ). The plasma and intracellular fluid are separated by the cell membrane, which we assume is permeable only to K+. (a) What is ∆G for the transfer of 1 mol of K+ from blood plasma to the cellular fluid at body temperature 37 °C?
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- For a certain chemical reaction, the equilibrium constant K = 2.7 × 10¹0 at 5.00 °C. Calculate the standard Gibbs free energy of reaction. Round your answer to 2 significant digits. AG° = [] kJ x10 X S ?arrow_forwardConsider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 2 M(s) +20₂(g) → M₂O4(s) For this reaction, AH = -4.961 kJ/mol and AS ixn = 12.12 J/(mol-K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGixn= What is the equilibrium constant of this reaction at 298 K? Kp = What is the equilibrium pressure of O₂(g) over M(s) at 298 K? MacBook Pro tyne URI + kJ/mol Oarrow_forwardA student determines the value of the equilibrium constant to be 6.29×104 for the following reaction.S(s,rhombic) + 2CO(g)SO2(g) + 2C(s,graphite)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 1.85 moles of S(s,rhombic) at standard conditions at 298K. G°rxn = _____ kJarrow_forward
- Calculate the standard change in Gibbs free energy, AGixn, for the given reaction at 25.0 °C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. KCI(s) K+ (aq) + Cl(aq) AGxn= Determine the concentration of K+ (aq) if the change in Gibbs free energy, AGran, for the reaction is -8.21 kJ/mol. [K+] = kJ/mol Marrow_forwardA student determines the value of the equilibrium constant to be 2.69×10-10 for the following reaction.Fe2O3(s) + 3H2(g)2Fe(s) + 3H2O(g)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank than zero.Calculate the free energy change for the reaction of 2.05 moles of Fe2O3(s) at standard conditions at 298K. G°rxn = ____kJarrow_forwardA student determines the value of the equilibrium constant to be 4.09×10-18 for the following reaction. Fe;O4(s) + 4H2(g)→3FE(s) + 4H,O(g) Based on this value of Kegi AG° for this reaction is expected to be (greater, less) greater than zero. Calculate the free energy change for the reaction of 1.76 moles of Fe;0,(s) at standard conditions at 298K. AG°. rxn = 190.5 kJarrow_forward
- Consider the oxidation of a generic metal M into a metal oxide as shown in the reaction. 3 2 M(s) + 0,(g) → M,O,(s) For this reaction, AHan -4.811 kJ/mol and ASirn = 12.06 J/(mol·K) at 298 K. What is the standard change in Gibbs free energy for the reaction in the forward direction? AGixn kJ/mol What is the equilibrium constant of this reaction at 298 K? Kp What is the equilibrium pressure of O,(g) over M(s) at 298 K? Ро, atmarrow_forwardEnter your answer in the provided box. Kf for the complex ion Ag(NH3)2+ is 1.5 × 107 at 25 ° C. Using this information, calculate the value of Δ G o f for Ag(NH3)2+(aq).arrow_forwardDetermine the molar ΔH°solution for a soluble ionic compound when the dissolution of 0.171 moles of that compound leads to a 12.9 °C temperature increase in a constant pressure calorimeter. The heat capacity of the calorimeter is 1.120 kJ/℃.arrow_forward
- ∆G ≤ 0 is an condition we use to indicate whether a reaction will proceed spontaneously and in what direction. (a) Show that this condition derives from the second law ofthermodynamics. (b) Explain when we can use ∆G for this purpose. (c) Explain why ∆G is oftenused instead of the entropy change.arrow_forward11. What is the ΔHº-value for the dissolution of NaOH (s) to yield 1.00... m NaOH (aq), given: Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (s) ΔHfº = -425.9 kJ/mol Na (s) + 1/2 O2 (g) + 1/2 H2 (g) → NaOH (aq, 1 m) ΔHfº = -469.2 kJ/mol Multiple Choice -895.1 kJ/mol -43.3 kJ/mol +1.102 kJ/mol +43.3 kJ/mol +895.1 kJ/molarrow_forward
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