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Calculate the enthalpy of solution (in kJ/mol) for dissolving 10.0 g of NaOH(s) in 100.0 g of water at 25°C, given that the final temperature of the solution is 28.5°C and the heat capacity of the solution is 4.18 J/g°C.

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

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Calculate the enthalpy change of reduction for Fe2O3 using the following data:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔH°rxn = -26.8 kJ mol^-1Fe2O3(s) + 2Al(s) → Al2O3(s) + 2Fe(l) ΔH°rxn = +824.2 kJ mol^-1Note: The standard enthalpy of formation for CO2(g) is -393.5 kJ mol^-1 and for Al2O3(s) is -1675.7 kJ mol^-1.

asked Jan 23 in ThermoChemistry by SGDJenifer99 (2.0k points)

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Calculate the enthalpy change of precipitation when 50 ml of 0.1 M silver nitrate (AgNO3) is added to 50 ml of 0.1 M sodium chloride (NaCl) solution. The temperature of the mixture increases by 5.0 °C. Given the specific heat capacity of the solution is 4.18 J/g °C and the density of the solution is 1.0 g/mL.

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

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Calculate the heat released when 1 mole of ethane (C2H6) is combusted in oxygen gas to form carbon dioxide and water, given the following enthalpy of combustion values: ΔH°comb(C2H6) = -1560 kJ/mol ΔH°comb(O2) = -393.5 kJ/mol ΔH°f(CO2) = -393.5 kJ/mol ΔH°f(H2O) = -285.8 kJ/mol

asked Jan 23 in ThermoChemistry by GingerJ92570 (1.6k points)

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Calculate the corrosion potential of a copper electrode immersed in a 1 M CuSO4 solution in contact with a silver electrode immersed in a 1 M AgNO3 solution. Given that the standard reduction potentials of Cu2+/Cu and Ag+/Ag are +0.34 V and +0.80 V, respectively. Determine which electrode will corrode and which electrode will act as a cathode in the galvanic cell.

asked Jan 23 in ElectroChemistry by HoraceT7712 (2.0k points)

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Calculate the bond order and bond length of the nitrogen-oxygen bond in nitric oxide (NO). Show your step-by-step work and include units in your answer.

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

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1 answer 58 views

Calculate the equilibrium constant, Kc, for the reaction:2SO2(g) + O2(g) ⇌ 2SO3(g) at a temperature of 600 K, given that the initial concentrations of SO2, O2, and SO3 were 0.025 M, 0.014 M, and 0 M, respectively, and at equilibrium [SO2] = 0.015 M, [O2] = 0.008 M, and [SO3] = 0.025 M.

asked Jan 23 in Chemical equilibrium by RandellBeggs (2.0k points)

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Calculate the melting and boiling points of Sodium Chloride (NaCl) using the Clausius-Clapeyron Equation given that the heat of fusion for NaCl is 28.9 kJ/mol, the heat of vaporization is 163.0 kJ/mol and the standard entropy change for phase transition is 72.14 J/K/mol.

asked Jan 23 in Inorganic Chemistry by ZKLBarbra368 (2.3k points)

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1 answer 65 views

Calculate the enthalpy of combustion of butane (C4H10) in kJ/mol given that its heat of formation value is -126.6 kJ/mol and the heat of formation values of CO2 and H2O are -393.5 kJ/mol and -241.8 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry by Karine04K24 (2.0k points)

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1 answer 67 views

Calculate the enthalpy change for the hydrolysis of sucrose given the following information: Sucrose (C12H22O11) reacts with water to form glucose (C6H12O6) and fructose (C6H12O6). Delta H for the reaction is -190 kJ/mol. The enthalpy of formation for sucrose is -2227 kJ/mol, the enthalpy of formation for glucose is -1274 kJ/mol, and the enthalpy of formation for fructose is -1266 kJ/mol.

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

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Calculate the Gibbs free energy change for the following reaction at 298 K: 2H2(g) + O2(g) → 2H2O(l) Given, ΔH = -483.6 kJ/mol and ΔS = -109.4 J/K/mol.

asked Jan 23 in Chemical thermodynamics by MariRosetta0 (2.2k points)

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Calculate the heat of hydration of MgSO4·7H2O if the enthalpy change for dissolving 1 mol of MgSO4 in water is -26.83 kJ/mol, and the enthalpy change for hydrating 1 mol of MgSO4·7H2O with 7 moles of water is -233.80 kJ/mol.

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

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1 answer 56 views

Calculate the heat of hydration of CuSO4.5H2O given that the enthalpy change for the reaction CuSO4.5H2O(s) -> CuSO4(s) + 5H2O(l) is -90.6 kJ/mol. Assume that the specific heat of the hydrated salt is 4.2 J/g*K and the density of the solution is 1.05 g/mL.

asked Jan 23 in ThermoChemistry by AmelieW70701 (1.7k points)

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1 answer 103 views

A student needs to calculate the standard enthalpy of formation of magnesium oxide, MgO, using Hess's Law. The student has access to the following reactions and their corresponding enthalpy changes:1. Mg(s) + 1/2O2(g) → MgO(s) ΔH = -601.8 kJ/mol2. Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH = -450.7 kJ/mol3. H2(g) + 1/2O2(g) → H2O(l) ΔH = -285.8 kJ/molWhat is the standard enthalpy of formation of MgO from its elements?

asked Jan 22 in ThermoChemistry by Marlene31P52 (2.5k points)

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1 answer 63 views

Calculate the enthalpy of formation for glucose (C6H12O6) at standard conditions, given the following enthalpies of formation for its constituent elements: C(graphite) = 0 kJ/mol H2(g) = 0 kJ/mol O2(g) = 0 kJ/mol Hint: Use Hess's Law and standard enthalpies of formation to solve the problem.

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

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1 answer 57 views

Calculate the formal charge on each atom in the nitrate ion (NO3^-).

asked Jan 23 in Inorganic Chemistry by WilheminaMea (1.5k points)

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1 answer 70 views

Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a copper electrode with a surface area of 25 cm² and a silver electrode with a surface area of 10 cm² for 3 hours. The half-cell potentials of copper and silver electrodes are +0.34 V and +0.80 V, respectively, and the molar concentrations of copper and silver ions in the electrolyte are 0.5 M and 1 M, respectively.

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

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1 answer 59 views

Calculate the enthalpy of vaporization for water if 50.0 g of water is completely vaporized at its boiling point (100°C) using 107 kJ/mol as the heat of vaporization of water.

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

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1 answer 69 views

Calculate the enthalpy change for the combustion of methane gas (CH4) if 37.0 g of CH4 is completely burned in a bomb calorimeter and the temperature increases by 285.4 K. Assume that the calorimeter has a heat capacity of 4.40 kJ/K and that the combustion reaction is as follows: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l); ΔH=-890.4 kJ/mol. What is the enthalpy change for the combustion of one mole of methane gas?

asked Jan 23 in Chemical reactions by RichieRedric (1.9k points)

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1 answer 65 views

Calculate the enthalpy change of the dissolution of 5 grams of sodium hydroxide (NaOH) in 100 mL of water, given the molar enthalpy of dissolution of NaOH to be -44 kilojoules per mole.

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

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