For the reaction\[ \text{CO(g) + 3H}_2\text{(g)} \rightarrow \text{CH}_4\text{(g) + H}_2\text{O(g)} \]\(\Delta H^\circ = -206.1 \, \text{kJ}\) and \(\Delta S^\circ = -214.7 \, \text{J/K}\)The standard free energy change for the reaction of 1.67 moles of \(\text{CO(g)}\) at 253 K, 1 atm would be \(\_\_\_\) kJ.This reaction is [ ] favored under standard conditions at 253 K.Assume that \(\Delta H^\circ\) and \(\Delta S^\circ\) are independent of temperature.

Answered: Image /qna-images/answer/f4410920-2baf-4c68-84ea-a94bc4e78317.jpg

For the reaction CO(g) + 3H₂(g) → CH₁ (9) + H₂O(g) AH = 206.1 kJ and AS° = -214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. kJ.

For the reaction CO(g) + 3H₂(g) → CH₁ (9) + H₂O(g) AH = 206.1 kJ and AS° = -214.7 J/K The standard free energy change for the reaction of 1.67 moles of CO(g) at 253 K, 1 atm would be This reaction is favored under standard conditions at 253 K. Assume that AH° and AS° are independent of temperature. kJ.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the maximum work that could be obtained at 25°C and 1 atm from the oxidation of 1.72 mol of aluminum by O₂(g) to give Al2O3(s). (The combustion of aluminum in booster rockets provides part of the energy that lifts the space shuttle off its launching pad, figure below) Blastoff of the space shuttle. Use data in the table below: Standard Free Energies of Formation of Typical Substances at 298.15 K AGI (kJ mol-¹) C₂H₂(g) C₂H4(g) C₂H6(g) C₂H₂OH() AG (kJ mol-¹) 0 -109.7 Substance Ag(s) AgCl(s) Al(s) Al₂O3(s) C(s) (graphite) CO(g) CO₂(g) CH4(g) -50.79 CH₂Cl(g) -58.6 CH₂OH(1) - 166.2 CO(NH,)2(s) -197.2 CO(NH2)z(aq) -203.8 +209 0.00 -1576.4 0 - 137.3 -394.4 +68.12 -32.9 -174.8 Substance CaO(s) -604.2 Ca(OH)2(s) -896.76 CaSO4(s) -1320.3 CaSO4 H₂O(s) -1435.2 CaSO4 2H₂O(s) -1795.7 Cl₂(g) 0 Fe(s) 0 Fe₂O3(s) H₂(g) H₂O(g) H₂O(1) HCI(g) HNO3(1) H₂SO4(!) HC,H,O,(0) Hg(1) -741.0 0 -228.6 -237.2 -95.27 -79.91 -689.9 -392.5 0 Substance K₂SO4(s) N₂(g) NH3(g) NH4Cl(s) NO(g) NO₂(g) N₂O(g) N₂O4(g)…
Calculate the free energy change for this reaction at 25 °C. Determine if +101.1 J/K. 1000 J the reaction is spontaneous? AH° = -2217 kJ; AS° = 1 kJ O -1161.1 kJ; the reaction is spontaneous O -2247 kJ; the reaction is spontaneous O +1161.1 kJ; the reaction is not spontaneous O +1864.2 kJ; the reaction is not spontaneous
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction.CaCO3(s) → CaO(s) + CO2(g) ΔG° = +131.1 kJP(CO2) = 0.033 atm
calculate the free energy change (in kJ) of a reaction at 466.4K that has an entropy change of 692.2J/K and an enthalpy change of -4.24kJ
Consider the reaction 2H2S(g) +302(g) =2H20(g) + 2SO2(g). If the standard free energy of the reaction is -976 kJ, what is the free energy in kJ of a reaction vessel containing 5.4 M H2S, 8.2 M O2, 2.1 M H2O, and 7.3 M SO2 at 298 K?
ΔG° for the reaction shown is equal to -419.6 (kJ/mol). Use the information given in the table to determine the standard free energy of formation vales, Gf° (kJ/mol) for the substance D. 1 A(s) + 1 B(g) → 1 C(s) + 1 D(g) Substance Gf°(kJ/mol) A(s) -684.3 B(g) -223.7 C(s) 187.7
At 560 K, /\G° = -21.3 kJ/mol for the reaction A (g) + 2 B (g) -> 3 C (g). If the partial pressures of A, B, and C are 0.420 atm, 0. 110 atm, and 7.20 atm respectively, what is the free energy for this reaction?
A key step in the production of sulphuric acid is the oxidation of SO2(g) + O2(g) → 2SO3(g) At 98K, ΔGosys = - 500.51kJ; ΔHosys = - 494.61. kJ; and ΔSosys = -60.16 J/K a) Use the data to decide if this reaction is spontaneous at 25°, and predicthow ΔGo will change with increasing T b) Assuming ΔHosys and ΔSosys are constant with increasing T, is the reaction spontaneous at 900oC?
The reaction A + B <> C has a molar DSrxn of -19 J/K and a molar DHrxn of 15 kJ. C has a free energy of formation of 10,000 kJ/mole, and B's free energy of formation is -3500 kJ/mole. What is the free energy of formation of A? Assume standard conditions, choose the closest. -7200 kJ/mole -5700 kJ/mole 7200 kJ/mole 5700 kJ/mole -34100 kJ/mole
For the reaction CO(g) + 3H2(g) → CH4(g) + H2O(g) AH = -206.1 kJ and AS° = -214.7 J/K The standard free energy change for the reaction of 1.52 moles of CO(g) at 253 K, 1 atm would be This reaction is reactant favored under standard conditions at 253 K. Assume that AH° and AS are independent of temperature. kJ.
For the reaction 2CO(g) + 2NO(g) → 2CO2 (g) + N2 (9) AH°=-746.6 kJ and AS° = -198.0 J/K The standard free energy change for the reaction of 2.36 moles of CO(g) at 275 K, 1 atm would be favored under standard conditions at 275 K. This reaction is Assume that AH° and AS are independent of temperature. Submit Answer Retry Entire Group '8 more group attempts remaining kj.
For a particular reaction, AH = 134.1 kJ/mol and AS = 35.0 J/(mol-K). Calculate AG for this reaction at 298 K. AG= What can be said about the spontaneity of the reaction at 298 K? The system is spontaneous in the reverse direction. The system is spontaneous as written. The system is at equilibrium. kJ/mol