need it asap plz 1) Consider the following reaction: CO(g) + H2O(g) + H2(g) + CO2(B)...
1.What is ΔGrxno (in kJ) at 440 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) 2. At what temperature (in K) does the above reaction become spontaneous?
1-What is ΔGrxno (in kJ) at 338 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) 2-At what temperature (in K) does the above reaction become spontaneous? PLEASE answer both
What is ΔGo (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) At what temperature (in K) does the above reaction become spontaneous?
7.H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.40 at 2000 K. (a) Calculate ΔG° for the reaction (b) Calculate ΔG for the reaction when the partial pressures arc PH2 = 0.25 atm, Pco2 = 0.78 atm. PH2O =0.66 atm. PCO 1.20 atm 8. Heating copper(II) oxide does not produce an appreciable amount of Cu. However if this reaction is coupled to the conversion of graphite to carbon monoxide, it becomes spontaneous. Write the coupled reaction and calculate its Delta G degree...
For the reaction Co (g) + 3 H2 (g)CH4(g) + H2O (g) calculate the enthalpy change in kJ at standard temperature and pressure for the consumption of 1.2 moles of carbon monoxide (g). The table below gives thermodynamic parameters. compound at 25 C ΔΗ f kj mol 'S JK ' mol kj mol carbon monoxide (g) -110.53 hydrogen (g) methane (g) water (I) water (g) 0 -1 197.67 130.68 186.26 69.95 188.83 137.17 74.81 285.83 241.82 -50.72 237.13 228.57 rxn...
use the following table for the reaction C2H2 (g) + 5/2 O2 (g) = 2CO2 (g) + H2O (g) delta H = -1255.5 KJ/mol substance S (J. mol-1. K-1) C2H2 (g) 200.8 C2H4 (g) 219.5 CO (g) 197.6 CO2 (g) 213.6 CO2 (aq) 117.6 H2O (l) 69.91 H2O (g) 188.7 O2 (g) 205.0 O (g) 161.0 O3 (g) 238.8 a. Use the data to calculate delta S in J/K for this reaction b. Calculate delta G in KJ , since the...
c) The standard enthalpies of formation and molar entropies of phosgene, carbon monoxide, and chlorine are COCl2(g): ΔfH° = -220.08 kJ mol-1; S° = 283.8 J mol-1 K-1 CO(g): ΔfH° = -110.53 kJ mol-1; S° = 197.66 J mol-1 K-1 Cl2(g): ΔfH° = 0 kJ mol-1; S° = 223.08 J mol-1 K-1 i) Determine the reaction Gibbs energy for the decomposition of phosgene at 298 K. Is this reaction spontaneous at this temperature? [25 marks] ii) At what temperature does...
for part a. for part b. thank you to who noticed! Consider the following reaction at 25 °C: 12 5 SO3(9) + 2 NH3(g) → 2 NO(g) + 5 SO2(g) + 3 H2O(9) a Given the information in the table, calculate AHº for the reaction. 1 point b Given the information in the table, calculate ASº for the reaction. 1 point с Determine the standard free energy for the reaction at 25°C. 1 point с Determine the standard free energy...
For the reaction CO(g) + H2O(1)—*CO2(g) + H2(g) AH° = 2.8 kJ and AS° = 76.8 J/K The standard free energy change for the reaction of 2.33 moles of CO(g) at 288 K, 1 atm would be kJ. This reaction is (reactant, product) favored under standard conditions at 288 K. Assume that AH° and ASº are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining For the reaction 2 NO(g) + O2(g) → 2 NO2(g) AG°...