delta G = Delta Go+RT ln Q
Part A. Using the following data, calculate Delta G at 298 K. Delta G (NO2(g))=51.84 kJ/mol. Delta G (NO2O4(g))=98.28 kJ/mol. Part B. Calculate Delta G at 298K if the partial pressures of NO2 and N2O4 are 0.36atm and 1.63atm, respectively. Please answer both questions Delta G in kJ format Next. Using the data from Appendix 4, calculate δG for the reaction below for the following conditions at 25°C. (Calculate all thermodynamic values from Appendix 4 for all parts of the problem.) kJ 2 H2S(g) + SO2(g) 3 Srhombic(s) + 2 H2O(g) PH2S = 1.0 10-4 atm PSO2 = 1.0 10-2 atm PH2O = 3.0 10-2 atm. Follow.1 answer 1.sing the data from Appendix 4, calculate δG for the reaction below for the following conditions at 25°C. (Calculate all thermodynamic values from Appendix 4 for all parts of the problem.). kJ. 2 H2S(g) + SO2(g) 3 Srhombic(s) + 2 H2O(g). PH2S = 1.0 10-4 atm. 1 Standard states for all species are 1 bar of partial pressure 25 °C. ( 2 This assumption matters a lot. 3  The meaning of the $^\circ$ symbol in $\Delta G^\circ$ can't be understood without it.4  The free energy of methanol liquid does not vary with pressure, i.e. $G_{liq} = G_{liq}^\circ$ at all pressures. will assume: 1  Methanol vapor is an ideal gas. 2  Standard states for all species are 1 bar of partial pressure 25 °C. ( 3 This assumption matters a lot. 4 I f need to calculate delta G using equation delta G =delta G not + R T ln Q. I am given partial pressure of the rxn as NO2 is 0.10 atm and N2O4 is 1 atm. I did Partial Pressure at 0,10 atm as 2.98 T for I mole NO2 and 298 K at STP for N2O4.  (b) 4.0 atm SO2, 2.0 atm O2, 10 atm SO3. (c) each reactant and product at a partial pressure of 1.0 atm. You need to use the following equation: delta G = delta G o + RT ln Q. where R is the Universal gas constant (8.31 J/molK), T is temp in Kelvin, and Q is the reaction quotient. An additional note for c. When the partial pressures are all equal to 1, Q = 1, and ln 1 = 0. Therefore, delta G = delta G o. This is not suprising because the standard delta G (delta G o)is by definition when the pressures are all equal to 1. Next. Calculate the change in free energy (KJ) for the reaction NO(g) + O3(g) → NO2(g) + O2(g) under the following conditions: T = 298 K ΔGo = -198.0 kJ/mol Pressure of NO = 1.06 x 10-5 atm Pressure of O3 = 1.44 x 10-5 atm Pressure of NO2 = 2.50 x 10-6 atm Pressure of O2 = 2.25 x 10-2 atm. 3 following. 1 answer. Report Abuse. Answers. Best Answer: use the formula delta G= -RTln K K=(partial pressure of NO2* partial pr of O2)/(partial pr of NO*partial pr of O3) R=8.314J. Source(s): periwinkle · 8 years ago. Thumbs up. 1 Use the equation PV = nRT to calculate the initial pressure of the SO 3 (g). 2  Use the equation pV = nRT to calculate the equilibrium partial pressure of the O 2 (g).inally, the equation Kp = Kc(RT) is used to calculate a value for Kp again, but this time from the value of Kc. Problem 2 involves calculating the equilibrium molar amounts of reactants and products, and then their partial pressures, from which a value for Kp can be obtained. Using the data from Appendix 4, calculate δG for the reaction below for the following conditions at 25°C. (Calculate all thermodynamic values from Appendix 4 for all parts of the problem.). kJ. 2 H2S(g) + SO2(g) 3 Srhombic(s) + 2 H2O(g). PH2S = 1.0 10-4 atm.
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calculate delta g using partial pressures