Calculate the standard Gibbs energy of the reaction at 298K, from the standard entropies and enthalpies of formation. CO(g) + CH3OH(l) yield CH3COOH(l)
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- Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().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 (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.
- 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.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?Calculate the standard reaction entropy and the standard Gibbs energy at 298 K of reaction 2CH3CHO(g) + O2(g) →2CH3COOH (l)
- 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.Calculate the standard reaction entropy at 298 K when 1 mol N2O(g) is formed from its elements in their reference states.Calculate the standard molar Gibbs energy of neon gas at 298 K.
- how to calculate the equilibrium constant given Delta Grxn= +6.4kJ/mol at 298KThe standard potential of the AgCl/Ag,Cl− couple fits the expressionE⦵/V = 0.23659 − 4.8564 × 10−4(θ/°C) − 3.4205 × 10−6(θ/°C)2 + 5.869 × 10−9(θ/°C)3Calculate the standard Gibbs energy and enthalpy of formation of Cl−(aq) and its standard entropy at 298 K.One reaction has a standard Gibbs energy of −320 kJ mol−1 and a second reaction has a standard Gibbs energy of −55 kJ mol−1, both at 300 K. What is the ratio of their equilibrium constants at 300 K?