Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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If we have a hydrophobic molecule in aqueous solution that makes contact with 25 water molecules, what is the change in molar Gibbs energy for adding this molecule into solution? Assume ΔH = 0 and T = 298 K.
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- Calculate the change in Gibbs energy for each of the sets of ΔrH∘, ΔrS∘, and T.arrow_forwardThe equilibrium constant for a system at chemical equilibrium at 318 oC is 3.4 x 10-3. Calculate the Gibbs free-energy change, deltaGo, for the system at 318 oC.Enter your answer here: kJ/molarrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4B(g) = 2C(g) + D(g) were found to be P = 4.62 bar, P = 4.70 bar, Pe=5.81 bar, and Pp = 5.90 bar. What is the standard change in Gibbs free energy of this reaction at 25 C? AG kJ/molarrow_forward
- For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N, (g) + 3 H, (g) = 2 NH,(g) the standard change in Gibbs free energy is AG° = –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.500 atm, PH, = 0.500 atm, and PNH, = 0.600 atm? AG = kJ/molarrow_forwardCalculate the change in the molar Gibbs energy of nitrogen gas when its pressure is isothermally increased from 1 atm to 1000 atm at 400 K. Based upon the calculated value of ΔGm, conclude if this process is spontaneous or not.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
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