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- Anda how about the standart potencial? E = Eº - 0,0591/n log kpsDetermine DG0 for the reaction:2CO(g) + 2H2(g) ---> CO2(g) + CH4(g)DH0 = -247.3 kJ/mol DS0 = -256.5 J/mol KThe oxidation of glucose to CO2 and water is a major source of energyin aerobic organisms. It is a reaction favored mainly by a large negativeenthalpy change. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(1) ΔH ° = -2816 kJ/mol ΔS ° = +181 J/mol • K(a) At 37 °C, what is the value for ΔG° ?(b) In the overall reaction of aerobic metabolism of glucose, 32 moles ofATP are produced from ADP for every mole of glucose oxidized. Calculatethe standard state free energy change for the overall reaction whenglucose oxidation is coupled to the formation of ATP at 37 °C.(c) What is the efficiency of the process in terms of the percentage of theavailable free energy change captured in ATP?
- The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a) Is it preferable to maintain this system at high or low pressure? Explain.At 25°c ,the thermodynamic equilibrium constant for reaction 3C2H2(g) converts into C6H6(l) is K=1.00 ×1088 and ITS ∆Hrxn=-631 KJ/mol .. CALCULATE ENTROPY CHANGE ∆Srxn in J/mol.k??
- For the reaction C(s) + CO2 (g) -> 2CO (g) determine kp and kc at 1000K and at 1100kFor the reaction 2 C6H5COOH(s) + 15 O2(g) → 14 CO2(g) + 6 H2O(g), ΔrU⦵ = −772.7 kJ mol−1 at 298 K. Calculate ΔrH⦵The value of Delta G at 261.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) +3Cl2 (g) -> 2PCI3 (g) is ___ kJ/mol. at 25.0oC for this reaction, delta H is -720.kJ/mol, Delta G is -642.9kJ/mol and delta s is -263.7 J/K
- Calculate the Delta Hrxn for the following reaction: C(s)+O2(g)--> CO2(g) DeltaHrxn=-393.5 kJ H2(g)+1/2O2(g)--> H2O (l) DeltaHrxn=-285.8 kJ C5H12(g)+8O2 (g)--> 5CO2(g) +6H2O(l) DeltaHrxn=-3536 kJ 10C(s)+12H2(g)-->2C5H12(g) DeltaHrxn=??????just to verify the answer rto 1 is increasing and 2 is increasing>??Calculate ΔG0reaction in kJ/mol at 298.15 K givenFe2O3(s)+3H2(g)→2Fe(s)+3H2O(l)ΔG^0reaction=ΣnΔG0Products−ΣnΔG0Reactants Substance ΔG0f (kJ/mol) ΔH0f(kJ/mol) S0298K (J/mol K) Fe2O3(s)Fe2O3(s) -742.2 -824.2 87.40 H2(g)H2(g) 0 0 130.7 Fe(s)Fe(s) 0 0 27.3 H2O(l)H2O(l) -237.1 -285.83 70.0 answer choices: a) 30.9 b)175.2 c)none of these d)158.7 e)-622.58
