Recent questions in Chemistry

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Calculate the Gibbs free energy change for the combustion of methane gas to produce carbon dioxide and water vapor at a temperature of 298K and a pressure of 1 atm, given the equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g) ΔG°f = -394.36 kJ/mol (CO2); ΔG°f = -237.13 kJ/mol (H2O); ΔG°f = -50.8 kJ/mol (CH4); ΔG°f = 0 kJ/mol (O2)

asked Jan 23 in Chemical thermodynamics by UNTChante96 (290 points)

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Calculate the Gibbs free energy change for the combustion of ethane gas in oxygen gas to form carbon dioxide gas and water vapor at a temperature of 25 °C and a pressure of 1 atm, given the following thermodynamic data:Reaction: C2H6(g) + 3.5O2(g) → 2CO2(g) + 3H2O(g)ΔH°rxn = -1560.8 kJ/molΔS°rxn = -283.3 J/K•molUsing the above information, what is the value of the Gibbs free energy change at standard conditions?

asked Jan 23 in Chemical thermodynamics by YasminDuncan (410 points)

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Calculate the Gibbs free energy change for the chemical reaction: 2H2O (l) → 2H2 (g) + O2 (g)at a temperature of 298 K, given that the standard Gibbs free energies of formation are ΔGf°(H2O) = -237.13 kJ/mol, ΔGf°(H2) = 0 kJ/mol, and ΔGf°(O2) = 0 kJ/mol.

asked Jan 23 in Chemical thermodynamics by AbdulCorser8 (290 points)

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Calculate the Gibbs free energy change at standard conditions for the reaction:2 H2(g) + O2(g) → 2 H2O(l)Given: ΔHºf[H2O(l)] = -285.8 kJ/mol, ΔHºf[H2(g)] = 0 kJ/mol, ΔHºf[O2(g)] = 0 kJ/mol, and ΔSº[H2O(l)] = -69.9 J/K·mol.

asked Jan 23 in Chemical thermodynamics by AidenChipman (250 points)

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Calculate the Gibbs free energy change at standard conditions for the following synthesis reaction: CO2 (g) + 2H2 (g) → CH3OH (g)

asked Jan 23 in Physical Chemistry by MatthewBouch (390 points)

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Calculate the Gibbs free energy change at standard conditions for the combustion of propane:C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) Given the standard enthalpy of formation data: ΔH°f(CO2(g)) = -393.5 kJ/mol ΔH°f(H2O(l)) = -285.8 kJ/mol ΔH°f(C3H8(g)) = -103.85 kJ/mol and the standard entropy data: S°(CO2(g)) = 213.6 J/(mol•K) S°(H2O(l)) = 69.9 J/(mol•K) S°(C3H8(g)) = 269.9 J/(mol•K)

asked Jan 23 in Chemical thermodynamics by LandonZfs700 (130 points)

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Calculate the Gibbs free energy change at 298 K for the reaction of hydrogen gas (H2) and chlorine gas (Cl2) to form hydrogen chloride gas (2HCl), given the following thermodynamic data:∆H°f (HCl) = -92.31 kJ/mol∆H°f (H2) = 0 kJ/mol∆H°f (Cl2) = 0 kJ/mol∆S°f (HCl) = -181.6 J/(mol*K)∆S°f (H2) = 130.7 J/(mol*K)∆S°f (Cl2) = 223.1 J/(mol*K)Also, determine whether the reaction is spontaneous at 298 K and if it will shift towards products or reactants.

asked Jan 23 in Chemical thermodynamics by LoydMyrick87 (520 points)

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1 answer 60 views

Calculate the Gibbs free energy change at 25°C for the reaction:2NO(g) + O2(g) → 2NO2(g)Given the standard Gibbs free energy of formation at 25°C for NO(g), O2(g), and NO2(g) are +86.4 kJ/mol, 0 kJ/mol, and +51.3 kJ/mol, respectively.

asked Jan 23 in Chemical thermodynamics by ChristianFar (290 points)

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Calculate the Gibbs free energy change (ΔG) for the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g)Given the standard Gibbs free energy of formation (ΔG°f) values at 298 K are:ΔG°f of NH3(g) = -16.6 kJ/molΔG°f of N2(g) = 0 kJ/molΔG°f of H2(g) = 0 kJ/molAssume ideal gas behavior for all gases involved in the reaction.

asked Jan 23 in Chemical thermodynamics by DorieBarth39 (510 points)

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Calculate the Gibbs free energy change (ΔG) for the reaction below at 298 K given the following standard Gibbs free energy of formation data: 2H2(g) + O2(g) → 2H2O(l) ΔG°f (kJ/mol): H2(g) = 0 O2(g) = 0 H2O(l) = -237.14

asked Jan 23 in Chemical thermodynamics by EdwardVmg820 (270 points)

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1 answer 46 views

Calculate the Gibbs free energy change (ΔG) for the following chemical reaction at 25°C and constant pressure of 1 atm:2H2(g) + O2(g) → 2H2O(l)Given the following standard Gibbs free energy of formation values (ΔfG°) at 25°C:H2(g) = 0 kJ/molO2(g) = 0 kJ/molH2O(l) = -237 kJ/mol

asked Jan 23 in Chemical thermodynamics by JonnieBonet (470 points)

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1 answer 45 views

Calculate the Gibbs free energy change (∆G) for the combustion of methane, CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l), at standard conditions (298 K and 1 atm pressure) using appropriate thermodynamic data.

asked Jan 23 in Chemical thermodynamics by CassieEdmist (350 points)

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Calculate the formal charge on the sulfur atom in the compound SO₃²⁻.

asked Jan 23 in Inorganic Chemistry by ValorieDemar (430 points)

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1 answer 51 views

Calculate the formal charge on the nitrogen atom in the molecule NO3-.

asked Jan 23 in Chemical bonding by Bradley53M38 (350 points)

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1 answer 55 views

Calculate the formal charge on each atom in the nitrate ion (NO3^-).

asked Jan 23 in Inorganic Chemistry by SimaBodenwie (210 points)

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1 answer 49 views

Calculate the formal charge on each atom in the molecule CO3^2-.

asked Jan 23 in Chemical bonding by MiaWelker055 (250 points)

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1 answer 46 views

Calculate the formal charge on each atom in SO4 2- ion.

asked Jan 23 in Inorganic Chemistry by RenePenningt (410 points)

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Calculate the formal charge of the sulfur atom in the sulfite ion (SO3) using the formula for formal charge calculation.

asked Jan 23 in Inorganic Chemistry by JoannaRtb513 (510 points)

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1 answer 51 views

Calculate the formal charge of the oxygen atom and the chlorine atom in the perchlorate ion, ClO₄⁻. Show your work and explain how you arrived at your answer.

asked Jan 23 in Inorganic Chemistry by MarcKohn2670 (430 points)

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1 answer 10 views

Calculate the formal charge of the nitrogen atom in the molecule NH3. Show your work and explain the significance of the result.

asked Jan 23 in Chemical bonding by RomanClaude4 (250 points)

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