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Concept explainers
Interpretation:
The Gibbs free energy and required change in enthalpy for a reaction system are to be calculated with given
Concept introduction:
Gibbs Free Energy can be defined as
Here,
When the change in entropy is negligible or zero, the equation changes to the expression:
Second law of thermodynamics tells about the spontaneity of a reaction and Gibbs free energy will tell in which direction the reaction is spontaneous.
It can be expressed mathematically as
Here,
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Chapter 3 Solutions
Organic Chemistry, 12e Study Guide/Student Solutions Manual
- to calculate the ΔH° of the unknown reaction:arrow_forward(28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forward(a) Write the chemical equation for the equilibriumthat corresponds to Kb. (b) By using the value ofKb, calculate ΔG° for the equilibrium in part (a). (c) What isthe value of ΔG at equilibrium? (d) What is the value of ΔGwhen [H+] = 6.7x 10-9 M, [CH3NH3 +] = 2.4 x 10-3 M,and [CH3NH2] = 0.098 M?arrow_forward
- (a) Calculate the standard free-energy change and the equilibrium constant for the dimerization of NO, to N2O4 at 25°C (see Appendix D). (b) Calculate AG for this reaction at 25°C when the pres- sures of NO2 and N,O4 are each held at 0.010 atm. Which way will the reaction tend to proceed?arrow_forwardWhat is the ΔGo for the following reaction from the equilibrium constant at the temperature given?arrow_forward3. (a) Use the data given below and calculate AHO, ASO, A Gº, and Kp at 25° C for the reaction: CO (g) + 3 H₂ (g) - → CH4 (g) + H₂O (g) (b) Calculate AG for the reaction at 250 °C. (c) At what temperature (°C) is AG equal to zero? In what temperature range is this reaction product- favored? Compound CO (g) H₂(g) CH4 (g) H₂O (g) AH°, kJ/mol -110.52 0 -74.81 -241.82 So, J/mol K 197.67 130.68 186.264 188.83arrow_forward
- Question: The following reaction reaches equilibrium at the specified conditions. C6H5CH=CH2 (g) + H2 (g) <---> C6H5C2H5 (g) The system initially contains 3 mol H2 for each mole of styrene. Assume ideal gases. For styrene, ΔGof,298 = 213.18 kJ/mol, ΔHof,298 = 147.36 kJ/mol. (a) What is Ka at 600oC? (b) What are the equilibrium mole fractions at 600oC and 1 bar? (c) What are the equilibrium mole fractions at 600oC and 2 bar? Request: Can you please help me with solving part c of this problem? You can go whichever order you want, but it is part c that I need help with the most. Thank you!arrow_forwardWith a ΔΔGo of -550.23 kJ, calculate the equilibrium constant for the reaction at 25.0 oC.arrow_forwardUsing S values from Appendix C, calculate AS values for the following reactions. In each case, account for the sign of AS. (a) C,H4(8) + H2(8) → C,H¿(8) (b) N,04(8) → 2 NO,(8) (C) Be(OH)2(s) (d) 2 CH;OH(8) + 302(g) → 2 CO2(8) + 4 H2O(g) BeO(s) + H,0(g)arrow_forward
- (a) For 1.00 mol of H2O(1) at 25 °C, what Ap is required to obtain a AG of +1.000 kJ? The molar volume of H2O(I) is 18.02 cm /mol. (b) For exactly 1 mol of ideal gas at 25 °C and 1.00 atm, what Ap is necessary to obtain a AG of +1.000 kJ? (c) Explain the difference in the two Ap values that you calculated.arrow_forwardThe reaction between NO2 and N2O4 is reversible. 2 NO2 (g) ⇌ N2O4 (g) For this reaction, ΔH o = -58.02 kJ/mol, and ΔS o = -176.6 J/mol-K. (a) What is the ΔGo at 25oC and 1 atm? (b) What is the equilibrium constant at 25oC and 1 atm? (c) What is the ΔG at 50oC if PNO2 =PN2O4 = 0.200 atm? Assume ΔH o and ΔSo are temperature independent (notes: the reaction will not be at equilibrium).arrow_forwardWhich statement is FALSE? (A) If a reaction is thermodynamically spontaneous it may occur slowly. (B) Activation energy is a kinetic quantity rather than a thermodynamic quantity. (C) If a reaction is thermodynamically spontaneous it may occur rapidly. (D) If a reaction is thermodynamically spontaneous, it must have a low activation energy. (E) If a reaction is thermodynamically nonspontaneous, it will not occur spontaneously.arrow_forward
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