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Calculate the enthalpy of combustion of ethanol (C2H5OH) if 45.1 g of ethanol is burned completely in excess oxygen, producing 145.5 kJ of heat energy.

asked Jan 23 in ThermoChemistry by RosettaMcinn (1.7k points)

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1 answer 85 views

Calculate the bond order and bond length of the CO molecule using molecular orbital theory.

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

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A chemistry student needs to determine the effect of increasing the temperature on the equilibrium constant of the formation of a complex ion. Given the equation: Fe3+ + 4OH- ↔ Fe(OH)4- Kc = 2.1 x 10^-18 If the initial concentration of Fe3+ is 0.02 M and OH- is 0.1 M at 25°C, what is the new equilibrium constant at 35°C assuming the reaction is exothermic and the heat of reaction is -20 kJ/mol?

asked Jan 22 in Chemical equilibrium by TimmyCapra21 (2.1k points)

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Calculate the equilibrium constant for the following electrochemical cell reaction at 25°C:Cu(s) + 2 Ag+(aq) --> Cu2+(aq) + 2 Ag(s)Given the standard reduction potentials are:Cu2+(aq) + 2 e- → Cu(s) E°red = +0.34 VAg+(aq) + 1 e- → Ag(s) E°red = +0.80 V

asked Jan 23 in ElectroChemistry by DeenaKuhn606 (2.0k points)

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1 answer 86 views

Calculate the average energy and specific heat capacity of a system containing 1000 molecules of an ideal gas at a temperature of 300 K, when the gas is subjected to an isochoric process and its volume remains constant at 2.5 L.

asked Jan 23 in Physical Chemistry by AOVFlorrie80 (1.7k points)

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1 answer 70 views

Calculate the Gibbs free energy change for the electrochemical reaction where Fe(s) is oxidized to Fe3+(aq) and Br2(l) is reduced to Br-(aq) with the help of the following half-reactions: Fe3+(aq) + e- ⇌ Fe2+(aq) E° = 0.771 VBr2(l) + 2e- ⇌ 2Br-(aq) E° = 1.087 V

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

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1 answer 71 views

Calculate the equilibrium constant at 25°C for the reaction: CO(g) + 3H2(g) ⇌ CH4(g) + H2O(g) If at equilibrium, the concentration of CO is 0.10 M, H2 is 0.20 M, CH4 is 0.015 M and H2O is 0.035 M.

asked Jan 23 in Chemical equilibrium by IsabellaOcto (1.9k points)

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1 answer 76 views

Calculate the enthalpy of ionization of magnesium using the following data: the first ionization energy of Mg is 738 kJ/mol and the lattice energy of MgCl₂ is -2495 kJ/mol.

asked Jan 23 in ThermoChemistry by Marlene31P52 (2.5k points)

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1 answer 125 views

A chemistry student is given an unknown compound and is required to identify its molecular structure using mass spectrometry. How can the student analyze the mass spectrum data to determine the compound's molecular weight and possible functional groups?

asked Jan 22 in Analytical Chemistry by WallaceMaria (2.4k points)

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1 answer 70 views

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 ChauFrederic (1.2k points)

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1 answer 76 views

Calculate the enthalpy of ionization for the reaction Mg(g) → Mg⁺(g) + e⁻ given that the ionization potential of Mg is 735 kJ/mol and the electron affinity of Mg⁺ is -195 kJ/mol.

asked Jan 23 in ThermoChemistry by PenneyMaxey5 (2.0k points)

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1 answer 79 views

Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)given that the enthalpy change of formation for water (H2O) is -285.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by TerrieGaffne (1.6k points)

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1 answer 158 views

What is the balanced equation for the oxidation of ethanol to acetic acid, and what is the reducing agent in this reaction?

asked Jan 21 in Organic Chemistry by PriscillaLaf (1.6k 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 ShanicePeele (2.0k points)

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1 answer 128 views

A 25 g sample of water at 25°C is heated by 200 J. The temperature of the water increases to 40°C. Calculate the specific heat capacity of water.

asked Jan 22 in Chemical thermodynamics by KariMcCleary (1.5k points)

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1 answer 79 views

Calculate the enthalpy change for the reaction below using Hess's Law: 2CO(g) + O2(g) -> 2CO2(g), delta H = -566 kJ/mol Given the following reactions and their corresponding enthalpy changes: CO(g) + 1/2O2(g) -> CO2(g), delta H = -283 kJ/molC(s) + O2(g) -> CO2(g), delta H = -393.5 kJ/mol

asked Jan 23 in ThermoChemistry by HalinaAlderm (1.9k points)

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1 answer 71 views

Calculate the equilibrium constant (K$\textsubscript{a}$) for the reaction of acetic acid in aqueous solution if the pH of the solution is 4.76 and the concentration of acetic acid is 0.1 M.

asked Jan 23 in Chemical equilibrium by ElidaHaskins (1.7k points)

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1 answer 69 views

Calculate the heat of formation of carbon dioxide gas (CO2) given the following bond energies: C=O bond energy is 799 kJ/mol and C-O bond energy is 358 kJ/mol.

asked Jan 23 in Chemical bonding by VanceW838771 (1.9k points)

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1 answer 78 views

Calculate the enthalpy change when 2 moles of nitrogen gas are adsorbed onto the surface of activated charcoal at a temperature of 298 K, given that the pressure of nitrogen is 1 atm and the final pressure of nitrogen adsorbed is 0.5 atm. The standard enthalpy of formation of nitrogen gas is 0 kJ/mol.

asked Jan 23 in ThermoChemistry by CherylDooley (1.7k points)

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1 answer 113 views

A student needs to prepare a solution containing 50 g of ethanol (C2H5OH) dissolved in 250 g of water (H2O) at 25°C. Assuming the heat of mixing for ethanol and water is -5.02 kJ/mol, calculate the heat released or absorbed when the two substances are mixed. Express your answer in kJ.

asked Jan 22 in ThermoChemistry by CarmineGaric (2.1k points)

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