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Calculate the standard enthalpy change for the dissolution of 5.36 g of NaOH in 100.0 mL of water, given that the molar enthalpy of dissolution for NaOH is -44.5 kJ/mol.

asked Feb 3 in Chemical thermodynamics by Eileen22S142 (1.7k points)

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Calculate the standard electrode potential for the redox reaction where Ag(s) is oxidized by Cu2+(aq) to form Ag+(aq) and Cu(s) given that the standard reduction potential for Ag+(aq) + e- → Ag(s) is 0.80 V and for Cu2+(aq) + 2e- → Cu(s) is 0.34 V.

asked Feb 3 in Chemical thermodynamics by TrevorE07525 (2.2k points)

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Calculate the standard enthalpy change for the vaporization of 25.0 g of water at 100°C, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol. (The molar mass of water is 18.015 g/mol.)

asked Feb 3 in Chemical thermodynamics by SterlingIsr (1.7k points)

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Calculate the standard enthalpy change for the reaction in which 25.0 mL of 0.100 M HCl(aq) is mixed with 25.0 mL of 0.200 M NaOH(aq) at 25°C. Assume that the specific heat capacity of the solution is 4.18 J/g⋅°C and that the density of both solutions is 1.00 g/mL.

asked Feb 3 in Chemical thermodynamics by CassieClopto (2.4k points)

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Calculate the standard enthalpy change for the dissolution of 5 grams of ammonium chloride (NH4Cl) in water, given that the molar enthalpy of dissolution of NH4Cl is -340.0 kJ/mol. The molar mass of NH4Cl is 53.49 g/mol and the density of water is 1.00 g/mL.

asked Feb 3 in Chemical thermodynamics by LSCJoey08837 (2.2k points)

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Calculate the standard enthalpy change for the vaporization of 10 grams of water at 100°C, given that the enthalpy of vaporization for water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by LeathaOchoa (1.7k points)

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Calculate the number of electrons transferred when a solution containing 0.25 M Ni(NO3)2 is electrolyzed using a current of 0.50 A for 2.0 hours. The reaction taking place is Ni2+ (aq) + 2e- --> Ni (s).

asked Feb 3 in ElectroChemistry by CooperPallad (1.7k points)

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Calculate the standard enthalpy change for the liquid-to-gas phase transition of water at 100°C and atmospheric pressure, given that the enthalpy of vaporization of water is 40.7 kJ/mol.

asked Feb 3 in Chemical thermodynamics by JoelPrentice (1.4k points)

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What is the effect of changing the concentration of the reaction intermediate on the overall rate of a chemical reaction?

asked Feb 3 in Chemical kinetics by DerrickKong0 (1.7k points)

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Calculate the standard enthalpy change for the reaction between 25 mL of 0.1 M HCl and 25 mL of 0.1 M NaOH, assuming the reaction takes place in aqueous solution and is complete. The temperature of the solutions should be maintained at a constant 25°C during the reaction. (Assume the density of the solutions is 1 g/mL and the specific heat capacity of the solutions is 4.18 J/g°C).

asked Feb 3 in Chemical thermodynamics by DieterSchrod (1.9k points)

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Consider a cell consisting of a zinc electrode in 1.0 M ZnSO4 solution and a copper electrode in 1.0 M CuSO4 solution. Calculate the standard cell potential of the cell at 25°C, given that the standard electrode potential for the zinc electrode is -0.76 V and for the copper electrode is +0.34 V.

asked Feb 3 in ElectroChemistry by StefanHartin (1.7k points)

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Calculate the standard enthalpy change for the fusion of 50 grams of ice at -10°C to liquid water at 10°C. Given the enthalpy of fusion of ice is 6.01 kJ/mol and the specific heat capacity of water is 4.184 J/g°C.

asked Feb 3 in Chemical thermodynamics by SheliaSaucie (2.1k points)

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Calculate the standard enthalpy of formation of carbon dioxide (CO2) using the following information:C(graphite) + O2(g) -> CO2(g), ΔH° = -393.5 kJ/molC(graphite) + 2H2(g) -> CH4(g), ΔH° = -74.8 kJ/mol2H2(g) + O2(g) -> 2H2O(l), ΔH° = -572.0 kJ/mol

asked Feb 3 in ThermoChemistry by AleidaSeifer (1.7k points)

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Chemistry student, can you predict the products and balance the following double replacement chemical reaction: NaCl + AgNO3?

asked Feb 3 in Chemical reactions by MiquelPlx868 (2.3k points)

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Calculate the standard Gibbs free energy change ($\Delta G^{\circ}$) for the following reaction at 298 K:2Fe(s) + 3/2O2(g) → Fe2O3(s) Given: Standard enthalpy of formation of Fe2O3(s) = -822.2 kJ/molStandard enthalpy of formation of Fe(s) = 0 kJ/molStandard entropy change for the reaction = +87.4 J/mol K

asked Feb 3 in Chemical thermodynamics by JackH2065356 (1.1k points)

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Calculate the standard free energy change, ΔG°, for the following redox reaction:2Fe2+ (aq) + H2O2 (aq) → 2Fe3+ (aq) + 2OH- (aq)Given the following half-reactions and their respective standard reduction potentials:Fe3+ (aq) + e- -> Fe2+ (aq) E° = +0.77 VH2O2 (aq) + 2H+ (aq) + 2e- ⟶ 2H2O (l) E° = +1.78 V

asked Feb 3 in Chemical thermodynamics by MacLgq130601 (2.4k points)

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Calculate the standard enthalpy of formation for propene (C3H6) given that the standard enthalpy of combustion of propene is -1411.1 kJ/mol and the standard enthalpy of formation of carbon dioxide (CO2) and water (H2O) are -393.5 kJ/mol and -285.8 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by Vern5918460 (2.5k points)

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Calculate the standard enthalpy change (ΔH°) for the reaction where 1 mol of solid sodium hydroxide (NaOH) dissolves in excess water to produce 1 mol of aqueous solution and releases heat. Given that the standard enthalpy of formation (ΔH°f) for NaOH(s) is -425.6 kJ/mol, the heat capacity of the aqueous solution is 4.18 J/gK, and the change in temperature (ΔT) is observed to be 8.0°C for 250 g of the solution.

asked Feb 3 in Chemical thermodynamics by MeredithFeg5 (1.6k points)

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Calculate the standard enthalpy change for the reaction: C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O (l)Given the following standard enthalpies of formation: ΔHf(C6H12O6 (s)) = -1273 kJ/molΔHf(CO2 (g)) = -393.5 kJ/molΔHf(H2O (l)) = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by SelenaRonan (2.2k points)

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Calculate the standard enthalpy change for the reaction: 2H2(g) + O2(g) → 2H2O(l)Given the standard enthalpies of formation are: ΔHf°(H2O(l)) = -285.8 kJ/mol ΔHf°(H2(g)) = 0 kJ/mol ΔHf°(O2(g)) = 0 kJ/mol Assume all reactants and products are at standard state conditions.

asked Feb 3 in Chemical thermodynamics by SimonMcWilli (1.9k points)

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