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Calculate the bond dissociation energy for the Cl-Cl bond in Cl2(g) given that the standard enthalpy change for the reaction Cl2(g) → 2 Cl(g) is +121 kJ/mol and the bond dissociation energy for the Cl-Cl bond in Cl2(g) is known to be 242 kJ/mol.

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

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1 answer 56 views

Calculate the enthalpy change for the oxidation of 25 grams of iron (Fe) to form iron(III) oxide (Fe2O3) using the balanced chemical equation and the given enthalpy of formation values for Fe(s) and Fe2O3(s).

asked Jan 23 in ThermoChemistry by EmmettVerdin (2.2k points)

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Calculate the bond order and bond length of the nitrogen-oxygen bond present in the nitrate ion (NO3-).

asked Jan 23 in Inorganic Chemistry by BarryEisenbe (2.3k points)

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Calculate the enthalpy of desorption for water molecules from the surface of a silica gel at a temperature of 25°C using the following information:- The vapor pressure of water at 25°C is 3.17 kPa.- The surface area of the silica gel is 25 cm².- The mass of the silica gel used in the experiment is 2.5 g.

asked Jan 23 in ThermoChemistry by JodieGartrel (1.8k points)

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Calculate the enthalpy change for the ionization of hydrogen atom if the ionization energy required is 1312 kJ/mol.

asked Jan 23 in ThermoChemistry by AngeliaDewey (1.8k points)

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Calculate the activation energy for a chemical reaction that has a rate constant of 0.007 mol/L/s at 25°C and 0.059 mol/L/s at 35°C.

asked Jan 23 in Chemical reactions by CheryleKirso (2.1k points)

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1 answer 47 views

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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Calculate the electronegativity difference between carbon and hydrogen in a methane (CH4) molecule using the Pauling scale of electronegativity.

asked Jan 23 in Chemical bonding by FerneSparks (2.3k 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 AngeliaDewey (1.8k points)

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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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Calculate the change in entropy and enthalpy for the reaction of iron (III) oxide with carbon monoxide to form iron and carbon dioxide, given the following information:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)ΔH°f (Fe2O3) = -824.2 kJ/molΔH°f (CO) = -110.5 kJ/molΔH°f (Fe) = 0 kJ/molΔH°f (CO2) = -393.5 kJ/molΔS° (Fe2O3) = 87.4 J/K molΔS° (CO) = 197.9 J/K molΔS° (Fe) = 27.3 J/K molΔS° (CO2) = 213.6 J/K mol

asked Jan 23 in Inorganic Chemistry by ShadArchie3 (1.7k points)

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Calculate the direction in which the equilibrium position will shift for the following reaction if the pressure is increased: N2(g) + 3H2(g) ⇌ 2NH3(g) ∆H° = -92.4 kJ/mol. Use Le Chatelier's principle to justify your answer.

asked Jan 23 in Chemical reactions by MontePlott51 (2.0k points)

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Calculate the equilibrium constant (K) of the electrochemical reaction below at 298K:Fe(s) + Cu2+(aq) ⇌ Fe2+(aq) + Cu(s) Given that at standard state (1 atm and 298K) the standard reduction potentials of Fe2+(aq)/Fe(s) and Cu2+(aq)/Cu(s) are -0.44 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by LibbyHollera (2.4k points)

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1 answer 46 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 FerminRosale (1.5k points)

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1 answer 54 views

Calculate the enthalpy change when 50 mL of 2 M HCl solution reacts with excess NaOH according to the balanced chemical equation: HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) Given that the specific heat capacity of the solution is 4.18 J/g°C, and the initial and final temperatures of the solution are 25°C and 35°C, respectively. Assume a density of 1 g/mL for the solution.

asked Jan 23 in Chemical reactions by WilheminaBel (2.0k points)

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1 answer 45 views

Calculate the heat of formation of methane (CH4) given the following thermochemical equations and standard heats of formation:2H2 (g) + O2 (g) → 2H2O (l) ΔH° = -572 kJ/molC (s) + O2 (g) → CO2 (g) ΔH° = -393.5 kJ/molNote: The standard heat of formation of CH4 is -74.8 kJ/mol.

asked Jan 23 in Chemical bonding by DominickPlum (2.5k 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 EloisaLeavit (1.5k points)

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1 answer 61 views

Calculate the bond dissociation energy of the O-H bond in a water molecule (H2O) given the enthalpy change for the reaction:H2O (g) → H2 (g) + 1/2 O2 (g)ΔH = +483.6 kJ/mol(Note: the bond dissociation energy represents the energy required to break a bond into its constituent atoms.)

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

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1 answer 100 views

A chemistry student needs to calculate the rate constant for the following reaction: 2 H2(g) + O2(g) --> 2 H2O(g) The initial concentration of H2 is 0.45 M and the initial concentration of O2 is 0.20 M. The reaction rate is measured to be 0.75 M/s. Calculate the rate constant for the reaction.

asked Jan 22 in Chemical kinetics by 43025337997 (2.2k points)

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Calculate the enthalpy change for the dissolution of 10 grams of sodium hydroxide in excess water, given that the solution formed has a final temperature of 25°C, and the specific heat capacity of the solution is 4.184 J/(g°C). The molar enthalpy of dissolution of NaOH is -44 kJ/mol. Assume that the density of the solution is equal to that of water.

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

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