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Calculate the bond length between two hydrogen atoms that are covalently bonded together. Given that the bond energy for the H-H bond is 436 kJ/mol and the force constant is 434 N/m.

asked Jan 23 in Chemical bonding by KWFErin73234 (1.9k points)

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1 answer 82 views

Calculate the anodic Tafel slope for an electrochemical cell in which the corrosion current density is 0.05 mA/cm² and the anodic overpotential is 50 mV. The exchange current density for the anodic reaction is 0.02 mA/cm².

asked Jan 23 in ElectroChemistry by OrvalLasley3 (2.1k points)

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1 answer 155 views

Identify the structural isomers for the alkane C6H14 and draw their structures, also name them according to IUPAC nomenclature.

asked Jan 21 in Organic Chemistry by HiramFarrell (1.7k points)

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1 answer 66 views

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 AngeliaDewey (1.8k points)

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1 answer 80 views

Calculate the change in entropy for the reaction: 2H2(g) + O2(g) → 2H2O(g)if the standard entropy values of H2, O2, and H2O are 130.7 J/mol*K, 205.0 J/mol*K, and 188.7 J/mol*K, respectively.

asked Jan 23 in Inorganic Chemistry by JoelPrentice (1.4k points)

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1 answer 76 views

Calculate the enthalpy change for the following reaction, using Hess's Law:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following enthalpy changes: 2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ2SO2(g) + O2(g) → 2SO3(g) ΔH2 = -198 kJ2H2(g) + S(s) → H2S(g) ΔH3 = +25kJ

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

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1 answer 67 views

Calculate the equilibrium constant (K) of the electrochemical reaction below at 25°C: 2AgCl(s) + H2(g) <--> 2Ag(s) + 2HCl(aq) Given: E°AgCl/Ag = 0.22 V E°HCl/H2 = 0.00 V Kw = 1.0 x 10^-14 at 25°C Standard Hydrogen Electrode (SHE) has E° = 0.00 V

asked Jan 23 in ElectroChemistry by QJXClarice2 (2.5k points)

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1 answer 66 views

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

asked Jan 23 in Inorganic Chemistry by VirgilioAbe5 (1.9k points)

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1 answer 74 views

Calculate the enthalpy change when 50 mL of water at 20°C is mixed with 30 mL of ethanol at 30°C. The specific heat capacity of water is 4.18 J g^-1 °C^-1, the specific heat capacity of ethanol is 2.44 J g^-1 °C^-1, and the density of both water and ethanol are 1 g/mL. Assume that the final mixture is at a uniform temperature.

asked Jan 23 in ThermoChemistry by Alejandra79W (1.9k points)

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1 answer 76 views

Calculate the enthalpy change for the following chemical reaction: 2NH3(g) + 3O2(g) → 2NO(g) + 3H2O(l) Given the following enthalpy values: ΔH°f (NH3) = −46.11 kJ/molΔH°f (O2) = 0 kJ/molΔH°f (NO) = 90.3 kJ/molΔH°f (H2O) = −285.8 kJ/mol

asked Jan 23 in Chemical thermodynamics by ShavonneSalc (1.8k points)

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1 answer 158 views

What is the IUPAC name of the following organic compound? CH3-CH2-CH(Cl)-CH=CH2Hint: The longest chain contains 5 carbon atoms.

asked Jan 21 in Organic Chemistry by MistyReagan2 (1.4k points)

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1 answer 79 views

Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a cell containing 0.150 L of a 0.250 M solution of CuSO4 for 2.00 hours. The cathodic half-reaction is Cu2+ + 2e- → Cu and the anodic half-reaction is Zn → Zn2+ + 2e-. The cell has a standard potential of 1.10 V at 298 K. What is the current density of the cell?

asked Jan 23 in ElectroChemistry by AmyNowland4 (2.5k points)

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1 answer 68 views

Calculate the enthalpy of vaporization of water at a temperature of 100 degrees Celsius and a pressure of 1 atm, given that the boiling point of water is 100 degrees Celsius and its enthalpy of vaporization at standard conditions (100 degrees Celsius and 1 atm) is 40.7 kJ/mol.

asked Jan 23 in ThermoChemistry by SOYRyan09176 (1.6k points)

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1 answer 81 views

Calculate the bond dissociation energy of the H-H bond in the H2 molecule. Given the bond length of H2 is 74 pm and the enthalpy change for the reaction H2(g) → 2H(g) is 436 kJ/mol.

asked Jan 23 in Chemical bonding by SoniaFanny4 (2.3k points)

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1 answer 75 views

Calculate the enthalpy change for the polymerization of propylene to polypropylene, given the enthalpy of formation of propylene is -103.8 kJ/mol and the enthalpy of formation of polypropylene is -45.4 kJ/mol. Assume the reaction occurs at constant pressure and temperature.

asked Jan 23 in ThermoChemistry by AlisiaBarwel (2.1k points)

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1 answer 83 views

Calculate the amount of heat absorbed or released when 2.5 moles of sodium acetate (NaCH3COO) is crystallized from its solution at a constant temperature of 25°C. The heat of crystallization for sodium acetate is -427 kJ/mol.

asked Jan 23 in ThermoChemistry by WayneYcs587 (2.5k points)

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1 answer 115 views

A chemistry student wants to see the effect of adding a specific buffer on the equilibrium position of a 0.1 M acetic acid (CH3COOH) and 0.1 M sodium acetate (CH3COONa) solution. If the initial pH of the solution is 4.7, what is the pH of the solution after adding the buffer? (Ka of acetic acid is 1.8 x 10^-5).

asked Jan 22 in Chemical equilibrium by AliceW140134 (2.0k points)

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1 answer 64 views

Calculate the heat released when 50 ml of 0.1 M HCl is neutralized with 50 ml of 0.1 M NaOH, assuming that the specific heat capacity of the mixture is 4.18 J/g°C and the density of the final solution is 1.0 g/mL.

asked Jan 23 in ThermoChemistry by Hanna191905 (2.0k points)

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1 answer 83 views

Calculate the amount of energy needed to desorb 10 moles of hydrogen gas from a metal surface, given that the enthalpy of desorption is -120 kJ/mol.

asked Jan 23 in ThermoChemistry by TiffaniWymar (1.6k points)

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1 answer 75 views

Calculate the enthalpy change for the isomerization reaction of butene-1 to cis-2-butene. Given that the standard enthalpy of formation for butene-1 is -19.8 kJ/mol and for cis-2-butene is -20.4 kJ/mol, and the standard enthalpy of combustion for butene-1 is -2876 kJ/mol.

asked Jan 23 in ThermoChemistry by TysonNettles (1.5k points)

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