Calculate the standard Gibbs energy of reaction for 4 HI(g) + O2(g) → 212(s) + 2H2O(1) at 298 K, using the values of standard entropies and enthalpies of formation given in the Resource section.
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A: Change in mole = 0.15 mmol Change in chemical potential = - 8.3 kJ/mol
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A: Gibbs energy change : ∆G = -nFE =- qE ∆G = -0.10 x 10-3 x 7.1 x 103 = -0.71 J
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- The standard enthalpy of combustion of liquid ethyl ethanoate (ethyl acetate, CH3COOC2H5) is −2231 kJ mol−1 at 298 K and its standard molar entropy is 259.4 J K−1 mol−1. Calculate the standard Gibbs energy of formation of the compound at 298 K.Calculate the standard Gibbs energy of reaction for 4 HI(g) + O2(g) → 2 I2(s) + 2 H2O(l) at 298 K, using the values of standard entropies and enthalpies of formation given in the Resource section.Calculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.
- The standard Gibbs energy of formation of PH3 (g) is 13.4 kJ/mol at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the H2 and PH3(treated as perfect gases) are 1.0 bar and 0.60 bar, respectively? What is the spontaneous direction of the reaction in this case?The standard enthalpy of combustion of the amino acid glycine (NH2CH2COOH) is -969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1 . Calculate the standard Gibbs energy of formation of glycine at 298 K.The standard Gibbs energy of formation of PH3(g) is +13.4 kJ mol−1 at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the H2 and PH3 (treated as perfect gases) are 1.0 bar and 0.60 bar, respectively? What is the spontaneous direction of the reaction in this case?
- For PbI2(s) ⇋ Pb2+(aq) + 2 I−(aq), K = 1.4 × 10−8 at 25 °C and the standard Gibbs energy of formation of PbI2(s) is −173.64 kJ mol−1. Calculate the standard Gibbs energy of formation of PbI2(aq).Calculate the change in the molar Gibbs energy of a perfect gas when its pressure is increased isothermally from 1.0 atm to 100.0 atm at 298 K.The standard Gibbs energy of formation of NH3(g) is −16.5 kJ mol−1 at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar, and 4.0 bar, respectively? What is the spontaneous direction of the reaction in this case?