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Calculate the change in entropy (ΔS) of the following reaction at 298 K:2SO2(g) + O2(g) → 2SO3(g) Given the standard molar entropies at 298 K: ΔS°(SO2,g) = 248.2 J/Kmol ΔS°(O2,g) = 205.0 J/Kmol ΔS°(SO3,g) = 256.2 J/Kmol

asked Jan 23 in Chemical thermodynamics by ChuWegener2 (2.1k points)

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Calculate the change in entropy (ΔS) for the reaction in which 3 moles of carbon monoxide (CO) gas is burned with excess oxygen gas to form 3 moles of carbon dioxide (CO2) gas. The reaction is carried out at constant pressure and a temperature of 298 K.

asked Jan 23 in Inorganic Chemistry by QJXClarice2 (2.5k points)

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Calculate the change in entropy (in J/K) for the following reaction at 298 K: 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) Given the following standard entropy values (in J/K): CH3OH (l): 126.6, O2 (g): 205.0, CO2 (g): 213.6, H2O (l): 69.9

asked Jan 23 in Chemical thermodynamics by RondaSkeyhil (1.7k points)

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Calculate the change in enthalpy for the reaction CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) given that the enthalpies of formation for CH4 (g), CO2 (g) and H2O (l) are -74.81 kJ/mol, -393.51 kJ/mol and -285.83 kJ/mol respectively.

asked Jan 23 in Physical Chemistry by CorneliusBur (2.1k points)

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Calculate the change in enthalpy for the following chemical reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given that the enthalpies of formation for CH4(g), CO2(g), and H2O(l) are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol respectively.

asked Jan 23 in Chemical reactions by ZKLBarbra368 (2.3k points)

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Calculate the change in enthalpy for the combustion of 2 moles of methane gas (CH4) at a constant pressure of 1 atmosphere and a temperature of 298 K. Given the standard enthalpy of formation for methane is -74.81 kJ/mol.

asked Jan 23 in Physical Chemistry by JadaMeece33 (1.6k points)

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Calculate the change in enthalpy and entropy for the reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) at 25°C given the following data:- ΔH°f for MgCl2(aq) = -641.3 kJ/mol- ΔS°f for MgCl2(aq) = -200.9 J/K/mol- ΔH°f for H2(g) = 0 kJ/mol- ΔS°f for H2(g) = 130.7 J/K/mol- ΔH°f for HCl(aq) = -167 kJ/mol- ΔS°f for HCl(aq) = -18.8 J/K/mol- ΔH°f for Mg(s) = 0 kJ/mol- ΔS°f for Mg(s) = 32.7 J/K/molAssume that ΔH°f and ΔS°f are independent of temperature.

asked Jan 23 in Inorganic Chemistry by ArleneLeichh (2.1k points)

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Calculate the change in enthalpy (ΔH) for the following reaction at 25°C given the standard enthalpies of formation for each compound: 2H2(g) + O2(g) → 2H2O(g) Standard enthalpies of formation: ΔHf° (H2O)(g) = -241.82 kJ/molΔHf° (H2)(g) = 0 kJ/molΔHf° (O2)(g) = 0 kJ/mol

asked Jan 23 in Physical Chemistry by TatianaSteil (2.3k points)

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Calculate the change in enthalpy (ΔH) for the combustion of methane gas (CH4) at 25°C and constant pressure of 1 atm. The equation for the combustion of methane is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) Given the standard enthalpies of formation at 25°C are:ΔHf[CH4 (g)] = -74.87 kJ/mol ΔHf[CO2 (g)] = -393.5 kJ/mol ΔHf[H2O (l)] = -285.8 kJ/mol Assume that water is in its liquid phase at the end of the reaction.

asked Jan 23 in Physical Chemistry by RobertoLafla (2.1k points)

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Calculate the change in enthalpy (ΔH) for the combustion of 10 grams of propane (C3H8) if the heat released by the reaction is -2202 kJ.

asked Jan 23 in Chemical reactions by AdelineBurro (1.9k points)

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Calculate the cell potential for the reaction:Hg2Cl2(s) + 2 Cl-(aq) → 2 Hg(l) + 2 Cl2(g)Given the standard reduction potentials: Hg2Cl2(s) + 2 e- → 2 Hg(l) + 2 Cl-(aq) E° = 0.268 VCl2(g) + 2 e- → 2 Cl-(aq) E° = 1.36 V

asked Jan 23 in ElectroChemistry by FletaStepp73 (2.0k points)

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1 answer 87 views

Calculate the cell potential for the reaction between a silver electrode and a copper electrode, given that the silver electrode is immersed in a 0.1 M AgNO3 solution and the copper electrode is immersed in a 1.0 M CuSO4 solution at 25°C. (Standard electrode potentials of Ag and Cu electrodes are +0.80 V and +0.34 V, respectively. Carry out the calculation in steps and provide the final answer with appropriate units.)

asked Jan 23 in ElectroChemistry by ChristieJzq (1.7k points)

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Calculate the cell potential for the following galvanic cell where a nickel anode is placed in a 1.0M Ni(NO3)2 solution and a silver cathode is placed in a 1.0M AgNO3 solution. The balanced equation for the cell reaction is: Ni(s) + 2 Ag+(aq) → Ni2+(aq) +2 Ag(s) Assume that standard reduction potentials for each half-reaction are as follows: Ni2+(aq) + 2 e- ⇌ Ni(s) E° = -0.25V Ag+(aq) + e- ⇌ Ag(s) E° = +0.80V What is the cell potential at standard conditions (25°C and 1 atm)?

asked Jan 23 in ElectroChemistry by GermanFranki (1.8k points)

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Calculate the cell potential for the following electrochemical reaction:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)Given that the standard reduction potentials for the half-reactions are as follows:Zn2+(aq) + 2e- → Zn(s) E° = -0.76 VCu2+(aq) + 2e- → Cu(s) E° = +0.34 V

asked Jan 23 in ElectroChemistry by TobiasTudawa (1.9k points)

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Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) The standard reduction potentials are: Cu2+(aq) + 2 e- → Cu(s) E° = 0.34 V Ag+(aq) + e- → Ag(s) E° = 0.80 V

asked Jan 23 in ElectroChemistry by FinleySalern (1.6k points)

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Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag⁺(aq) → Cu²⁺(aq) + 2 Ag(s) Given that the standard reduction potentials are: Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

asked Jan 23 in ElectroChemistry by AundreaWhitf (1.8k points)

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1 answer 73 views

Calculate the cell potential for the following electrochemical reaction at 25°C: Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) Given: E°(Ag+/Ag) = +0.80 V E°(Zn2+/Zn) = −0.76 V

asked Jan 23 in ElectroChemistry by Lynell160113 (1.8k points)

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1 answer 89 views

Calculate the cell potential for a given electrochemical reaction where the half-cell reactions are:* Fe3+(aq) + e- → Fe2+(aq) E° = 0.77 V* Ag+(aq) + e- → Ag(s) E° = 0.80 VAssume 1.0 M solutions and standard state conditions. Determine whether the reaction is spontaneous or non-spontaneous under standard conditions.

asked Jan 23 in ElectroChemistry by AntoniettaLa (1.9k points)

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Calculate the cell potential at standard conditions for the electrochemical reaction: Cu(s) + 2Ag+(aq) -> 2Ag(s) + Cu2+(aq) given that the standard reduction potentials for Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) are +0.34 V and +0.80 V, respectively.

asked Jan 23 in ElectroChemistry by MoniqueBrins (1.9k points)

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Calculate the bond order of the nitrogen molecule (N2) using molecular orbital theory.

asked Jan 23 in Physical Chemistry by LorenzoWooll (1.7k points)

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