Answer: Δ H = 65 kJ/mol ——> 65000 J/mol. What information are we given? Delta G = -nFE = - (1 moles e-) (96,485 J/mol e-volt) (1.27 volts) dG = -122,535.95 J = … Chemistry Calculate delta G of the reaction at 25 degrees C: 2Au^3+ (aq) + 3Ni(s) 2Au(s) + 3Ni^2+(aq) Au3+ + 3e- ==> Au Eo = +1.50V Ni2+ + 2e- ==> Ni Eo = -0.23 V 2Au3+ + 3Ni ==> 3Ni2+ + 2Au The answer is -1.00 x 10^3 kJ but i'm not getting that answer!!!!!!! Use standard free energies of formation to calculate Delta G degree at 25 degree C for each of the following reactions. Calculating the (Gibbs) Free Energy of Formation for the Reaction the equation is (delta G)=(delta G^0)+RTlnK Delta G^0= (Delta G^0 of goods - reactants) R=8.312/one thousand T=must be in kelvin ok= (rigidity of goods)/(rigidity of reactants) (PH2^2 x PCO)/ PCH3OH evaluate the reaction: CH3OH(g)?CO(g)+2H2(g) Calculate ?G for this reaction at 25 ?C under those situations: PCH3OH= 0.840atm PCO= 0.145atm PH2= 0.195atm I had diverse numbers and that … Pccl4 = 0.174 atm. SBra(gS(g)+2Br2(0) +152 kJ -56.7 kJ +77.8 kJ +37.1 kJ Using E° values given below, calculate delta G° at 25°C for the cell Fe/ Fe2+ // Cu2+ / Cu under standard conditions will be : Data Fe2+ + 2e- Fe°; E° = - 0.44 V Cu2+ + 2e- Cu°; E° = 0.34 V Please don't just give me the answer, i need to learn how to do it i.e. For example, if your reaction is at 350K and your table is for 298K then for each reactant and product the enthalpy and entropy of formation is: Delta_fH_350 = Delta_fH_298 + C_P(350-298) S_350 = S_298 + C_P ln(350/298) Then calculate the DeltaH and DeltaS for the reaction and the rest of the procedure is unchanged. CO2 (g) + CCl4 (g) <--> 2 COCl2 (g) Calculate delta G for this reaction at 25 C? Favorite Answer. Write the balanced equation for the combustion of methanol and solve for Delta G rxn, Delta H rxn and delta S rxn at 25 C. Is the reaction spontaneous? please tell me what i'm substituting incorrectly. Calculate delta G for the reaction below at a temperature of 25°C, given that ΔH° = 52.96 kJ and ΔS° = 166.4 J/K. Relevance. VIDEO Calculate Δ G (DELTA G) Demonstrated Example 4: A chemical reaction has the Δ H of 65 kJ/mol the temperature of -100 C and the Δ S of 14 J/mol K. What is the Gibbs free energy? 3 Answers. I … Pcocl2 = 0.744 atm. Calculate the delta G for the reaction at 25 C For the following reaction at 25°C, A Ho = +115 kJ and A S= +125 J/K. Calculate Delta G for this reaction at 25 degrees C under the following conditions: Pressure of CH3OH = 0.890 atm P CO = 0.120 atm P H2 = 0.175 atm CH3OH (g) <-> CO(g) +2H2(g… 10 years ago. the equation is (delta G)=(delta G^0)+RTlnK Delta G^0= (Delta G^0 of things - reactants) R=8.312/one thousand T=must be in kelvin ok= (stress of things)/(stress of reactants) (PH2^2 x PCO)/ PCH3OH evaluate the reaction: CH3OH(g)?CO(g)+2H2(g) Calculate ?G for this reaction at 25 ?C lower than those circumstances: PCH3OH= 0.840atm PCO= 0.145atm PH2= 0.195atm I had diverse … the steps to follow as this type of question will probably be in my upcoming exam. Please help :] Answer Save. Under these conditions : Pco2 = 0.112 atm. For the reaction described by the chemical equation: 3C2H2(g) -> C6H6(l) .. Delta H rxn = -633.1 kJ/mol a) Calculate the value of Delta S rxn at 25.0 C... b) Calculate Delta G rxn... c) In which direction is the reaction, as written, spontaneous at 25 C . H2(g) + I2(g) → 2HI(g) Please show step by step instructions, thanks Expert Answer T = -100 C ——> 173 K Is this reaction spontaneous or non-spontaneous? Steve O. Lv 7.