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Calculate the Gibbs free energy change for the electrochemical reaction in which 2 moles of electrons are transferred from a zinc electrode to a copper electrode. The standard reduction potentials are E°(Cu²⁺/Cu) = 0.34 V and E°(Zn²⁺/Zn) = -0.76 V. What is the spontaneity of the reaction under standard conditions?

asked Jan 23 in ElectroChemistry by BuckY7205505 (1.7k points)

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Calculate the bond length between a hydrogen atom and an oxygen atom in an H2O molecule, given that the hydrogen-oxygen bond energy is 463 kJ/mol and the reduced mass of the two atoms is 1.6735 x 10^-27 kg.

asked Jan 23 in Chemical bonding by JuanitaPiess (2.1k points)

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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 GroverRamey (2.2k points)

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Calculate the equilibrium constant (K) for the electrochemical reaction: Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s) Given that the standard reduction potentials for Ag+ and Mg2+ are +0.80 V and -2.37 V, respectively. The concentration of Ag+ is 0.020 M and the concentration of Mg2+ is 0.080 M.

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

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Calculate the enthalpy change when 2.5 moles of methane gas is completely burned in excess oxygen gas if the enthalpy of formation of methane is -74.8 kJ/mol and the enthalpy of formation of water is -285.8 kJ/mol, and the enthalpy of formation of carbon dioxide is -393.5 kJ/mol.

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

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Calculate the enthalpy change for the precipitation reaction of barium chloride and sodium sulfate, given that the initial concentrations of the two solutions are 0.2 M and are mixed in a coffee cup calorimeter. The final temperature observed is 25°C and the heat capacity of the coffee cup is 10 J/°C.

asked Jan 23 in ThermoChemistry by ErikaStephen (2.4k points)

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Calculate the irreversible work done by a gas expanding adiabatically from an initial volume of 1 L to a final volume of 5 L against a constant external pressure of 2 atm, assuming that the gas is initially at a temperature of 300 K and that its final temperature is 400 K.

asked Jan 23 in Physical Chemistry by AngeliaDewey (1.8k points)

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Calculate the corrosion potential of a zinc-copper galvanic couple in which the zinc electrode has a concentration of 0.1 M and the copper electrode has a concentration of 0.01 M. The standard reduction potentials for Zn2+/Zn and Cu2+/Cu are -0.76 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by MAQShelton1 (1.7k points)

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Calculate the heat of combustion for propane gas, C3H8(g), if 12.5 grams of propane are completely burned in excess oxygen gas and the products of reaction are cooled from 700°C to 25°C. The heat capacities of the reactants and products are as follows: C3H8(g): cp = 44.10 J/K O2(g): cp = 29.38 J/K CO2(g): cp = 36.8 J/K H2O(g): cp = 33.6 J/K Assume that the heat capacities of the products and reactants are constant over the temperature range of the reaction and that the heat lost to the surroundings is negligible.

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

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Calculate the exchange current density for a redox reaction where the standard potential is 0.7 V, and the transfer coefficient is 0.5, given that the rate constant for the reaction is 5 × 10^-7 mol/cm^2*s.

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

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Calculate the heat of mixing when 50g of ethanol (C2H5OH) is added to 200g of water initially at 25°C. Assume the density of water is 1g/mL and the specific heat capacity of water is 4.184J/(g°C). The enthalpy of vaporization of ethanol is 38.56kJ/mol and assume that ethanol-water mixture has a specific heat capacity of 4.2J/(g°C).

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

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Calculate the heat capacity of 10 grams of water if the temperature of the water increases by 5°C upon absorption of 200 Joules of heat.

asked Jan 23 in Chemical thermodynamics by BradlySyr093 (1.8k points)

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Calculate the mass of silver (Ag) that will be deposited on the cathode during electrolysis if a current of 2.5 A is passed through a solution of silver nitrate (AgNO3) for 3 hours.

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

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Calculate the enthalpy change for the reduction of iron (III) oxide using carbon in a thermite reaction if 12.5 grams of iron (III) oxide reacts with excess carbon, and the resulting iron has a mass of 7.5 grams. Assume all heat evolved is absorbed by the iron and that the reaction occurs at constant pressure.

asked Jan 23 in ThermoChemistry by SusannahRose (1.3k points)

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1 answer 79 views

Calculate the amount of heat required to raise the temperature of 50 g of water from 25°C to 100°C, given the specific heat capacity of water is 4.18 J/g°C.

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

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1 answer 68 views

Calculate the enthalpy of formation of NaCl(s) using the following information:1. The enthalpy change of formation of Na(g) is +108.5 kJ/mol.2. The enthalpy change of formation of Cl2(g) is 0 kJ/mol.3. The enthalpy change of vaporization of Na is +97.42 kJ/mol.4. The enthalpy change of dissociation of Cl2 is +242.76 kJ/mol.

asked Jan 23 in ThermoChemistry by MarcellaR325 (2.2k points)

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Calculate the lattice energy of magnesium oxide (MgO) given that the ionic radii for Mg2+ and O2- are 0.72 Å and 1.40 Å respectively, and the lattice energy of MgO is -3795 kJ/mol.

asked Jan 23 in Inorganic Chemistry by MOIRoderick9 (1.8k points)

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Calculate the enthalpy of solution for 10.0 g of potassium chloride (KCl) dissolved in 100 mL of water, given that the temperature of the solution decreases from 25°C to 20°C. Assume the heat capacity of the solution to be 4.184 J/g°C and that there is no heat loss to the surroundings.

asked Jan 23 in ThermoChemistry by MontePlott51 (2.0k points)

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Calculate the enthalpy change of solution for 5.00 g of ammonium chloride (NH4Cl) dissolved in 50.0 mL of water, given that the temperature of the solution decreases by 4.21°C. The density of water is 1.00 g/mL and the specific heat capacity of the solution is 4.18 J/g°C. The molar mass of ammonium chloride is 53.49 g/mol.

asked Jan 23 in ThermoChemistry by Miguel37A006 (2.3k points)

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Calculate the heat capacity of 50g of water when its temperature is raised from 25°C to 65°C.

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

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