Recent questions in ThermoChemistry

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Here's a precise problem for a chemistry student to solve, based on Thermochemistry and the Enthalpy of Desorption Calculations:Given the following data for the adsorption of hydrogen gas on a metal surface:- Initial pressure of hydrogen gas = 1 atm- Final pressure of hydrogen gas after adsorption = 0.2 atm- Temperature = 298 K- Surface area of the metal = 5 cm^2- Enthalpy of Desorption of hydrogen gas on the metal surface = -40 kJ/molCalculate the enthalpy change (in kJ) for the adsorption of hydrogen gas on the metal surface.

asked 23 hours ago in ThermoChemistry by HattieSteven (310 points)

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Given the following information: A polymerization reaction has a heat of reaction of -150 kJ/mol and a Δn (change in moles of gas) of +2 moles gas/mol. If 5.0 g of the monomer is polymerized, what is the enthalpy change (in kJ) for the overall reaction?

asked 23 hours ago in ThermoChemistry by LucileSams37 (390 points)

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Given the enthalpy of solution of sodium hydroxide (NaOH) is -44.5 kJ/mol and the enthalpy of solution of hydrochloric acid (HCl) is -74.8 kJ/mol, calculate the enthalpy change for the precipitation reaction between NaOH and HCl, assuming all solutions are at a concentration of 1 M.

asked 23 hours ago in ThermoChemistry by MeghanIliffe (430 points)

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Given the balanced chemical equation: C6H12O6 + 6O2 -> 6CO2 + 6H2O The enthalpy of formation of glucose is -1273 kJ/mol and the enthalpy of formation of water is -286 kJ/mol. Calculate the enthalpy change of the oxidation of glucose in kJ/mol.

asked 23 hours ago in ThermoChemistry by KianUlt79673 (330 points)

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1 answer 39 views

Given that the enthalpy of vaporization of water is 40.7 kJ/mol at its boiling point of 100°C, calculate the amount of energy required to boil 500g of water starting from 25°C.

asked 23 hours ago in ThermoChemistry by IslaWoodward (530 points)

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1 answer 45 views

Given a sample of dry ice (solid CO2) with a mass of 50 grams, calculate the amount of heat energy that needs to be added to sublimate it completely into gaseous CO2 at a temperature of -78.5°C. The heat of sublimation of CO2 is 25.2 kJ/mol. (Assume that CO2 is an ideal gas under these conditions.)

asked 23 hours ago in ThermoChemistry by Shari7998231 (600 points)

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Determine the standard enthalpy of formation for ammonium chloride (NH4Cl) using Hess's Law and the following given reactions: 1) N2(g) + 3H2(g) → 2NH3(g) ΔH° = -46.0 kJ/mol 2) NH3(g) + HCl(g) → NH4Cl(s) ΔH° = -176.2 kJ/mol 3) N2(g) + 2H2(g) + 2Cl2(g) → 2NH4Cl(s) ΔH° = -634.2 kJ/mol

asked 1 day ago in ThermoChemistry by EddieWhittin (490 points)

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1 answer 23 views

Determine the heat of hydration, in kJ/mol, for the reaction between solid Calcium chloride (CaCl2) and water (H2O), given that 1 mole of CaCl2 dissolves to produce 3 moles of ions and releases -82.8 kJ of heat in the process.

asked 1 day ago in ThermoChemistry by ErnestoSprou (470 points)

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1 answer 31 views

Determine the enthalpy of hydrolysis for sodium acetate (NaC2H3O2) given that the enthalpy of neutralization for acetic acid (HC2H3O2) and sodium hydroxide (NaOH) is -55.9 kJ/mol and the heat of formation for NaC2H3O2 is -382.7 kJ/mol.

asked 1 day ago in ThermoChemistry by OliverY88898 (370 points)

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1 answer 16 views

Determine the enthalpy of desorption for carbon dioxide from activated charcoal at 25°C. Given: the equilibrium pressure of CO2 is 0.1 atm and the mass of charcoal used is 2.5 g.

asked 1 day ago in ThermoChemistry by CatalinaBerg (630 points)

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1 answer 39 views

Determine the enthalpy of adsorption for the reaction of hydrogen gas adsorbing onto a platinum surface, given that 2.00 g of hydrogen gas is adsorbed onto a 1.00 g platinum surface at 25°C and the pressure is 1 bar. The volume of the system is 1.00 L and the initial temperature of the platinum surface is also 25°C. Assume that the surface is in thermal equilibrium with the surroundings and that the gas behaves ideally.

asked 1 day ago in ThermoChemistry by TeresitaJack (450 points)

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1 answer 37 views

Determine the enthalpy change of precipitation for the reaction between 50ml of 0.1M sodium sulfate and 50ml of 0.1M barium nitrate, given that the final temperature is 25°C and the initial temperature was 30°C. The specific heat capacity of the solution is 4.18 J/g °C and the density is 1 g/mL. (Assume the reaction goes to completion and all volumes are additive.)

asked 1 day ago in ThermoChemistry by MerleSundber (430 points)

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1 answer 36 views

Determine the enthalpy change of precipitation for the reaction between 50 mL of 0.1 M NaOH and 50 mL of 0.1 M CuSO4, given that the final solution has a temperature of 25°C and the specific heat capacity of the solution is 4.18 J/g·°C.

asked 1 day ago in ThermoChemistry by EarleFrye28 (330 points)

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1 answer 30 views

Determine the enthalpy change for the oxidation of 2 moles of iron (Fe) to form iron oxide (FeO) using the following data: Fe + 1/2 O2 → FeO ΔH = -65.0 kJ/mol 4 Fe + 3 O2 → 2 Fe2O3 ΔH = -1648.6 kJ/mol

asked 1 day ago in ThermoChemistry by JeffrySchuhm (390 points)

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1 answer 21 views

Determine the bond dissociation energy of methane (CH4) using the following data: Reaction: CH4(g) → C(g) + 4H(g)ΔH°f (kJ/mol): CH4(g) = -74.81C(g) = 715.32H(g) = 218.00Hint: bond dissociation energy can be calculated using the formula ΔH°rxn = Σ (ΔH°f, products) - Σ (ΔH°f, reactants)

asked 1 day ago in ThermoChemistry by ReyesBoettch (610 points)

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1 answer 4 views

Consider the following reactions:1. Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) ΔH₁ = -454.9 kJ/mol2. MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂O(l) ΔH₂ = -131.3 kJ/mol3. H₂(g) + ½O₂(g) → H₂O(l) ΔH₃ = -285.8 kJ/molUsing Hess's Law, calculate the enthalpy change for the following reaction:MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g) given that the enthalpy change for the reaction Mg(s) + ½O₂(g) → MgO(s) is ΔH = -601.6 kJ/mol.

asked 1 day ago in ThermoChemistry by CallieMargar (550 points)

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1 answer 28 views

Calculate the total heat change when 100 ml of 0.5 M HCl is mixed with 100 ml of 0.5 M NaOH at 25°C. Assume the heat capacity of the solution is 4.18 J/(g°C) and the density of the solution is 1 g/mL. The enthalpy of neutralization of HCl and NaOH is -57.3 kJ/mol.

asked 1 day ago in ThermoChemistry by IsabellSchul (490 points)

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1 answer 39 views

Calculate the standard heat of mixing when 50 mL of 1 M HCl is mixed with 100 mL of 1 M NaOH at 25°C. The standard heat of neutralization of 1 M HCl and 1 M NaOH is -57.32 kJ/mol.

asked 1 day ago in ThermoChemistry by CarmelaMonte (510 points)

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1 answer 17 views

Calculate the standard enthalpy of reduction for the following reaction: Fe2O3 (s) + 3 H2(g) → 2 Fe(s) + 3 H2O(g)Given: ΔH°f for Fe2O3 (s) = -824.2 kJ/mol ΔH°f for H2O(g) = -241.8 kJ/molΔH°f for Fe(s) = 0 kJ/mol

asked 1 day ago in ThermoChemistry by TiaraTraill (390 points)

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1 answer 22 views

Calculate the standard enthalpy of precipitation for the reaction: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) given that the standard enthalpies of formation for AgNO3(aq), NaCl(aq), AgCl(s), and NaNO3(aq) are -123.2 kJ/mol, -407.3 kJ/mol, -127.0 kJ/mol, and -467.3 kJ/mol, respectively.

asked 1 day ago in ThermoChemistry by DarciPok795 (530 points)

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