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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Organic Chemistry
- (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(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_forwardto calculate the ΔH° of the unknown reaction:arrow_forward
- What 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_forwardWith a ΔΔGo of -550.23 kJ, calculate the equilibrium constant for the reaction at 25.0 oC.arrow_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_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_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_forward
- Which 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(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_forward1. The depletion of ozone in the stratosphere can be summarized by this equation: 203(g) 302(g) O3(g) O2(g) AH°f 142.7 kJ/mol 0 So 239 J/K.mol 205 J/K-mol (i) Calculate AS° and AG° for this reaction. (ii) Calculate the equilibrium constant. (iii) Explain, in molecular terms, the sign of AS° for this equilibrium. (iv) What is the significance of your answers with respect to ozone depletion? (v) How would you expect the value of AG to change with increasing temperature? Explain.arrow_forward
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