Hot questions

0 votes

1 answer 63 views

Calculate the enthalpy of desorption of CO2 from sodium hydroxide (NaOH) pellets given the following information: - The heat of absorption of CO2 by NaOH pellets is -20.9 kJ/mol.- The standard enthalpy of formation of Na2CO3 is -1130 kJ/mol.- The standard enthalpy of formation of water is -286 kJ/mol.- The standard enthalpy of formation of NaOH is -425 kJ/mol. Assuming that the desorption process is the reverse of the absorption process, determine the enthalpy change for the reaction: Na2CO3(s) + H2O(l) → 2NaOH(s) + CO2(g).

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

0 votes

1 answer 63 views

Calculate the enthalpy of desorption of carbon dioxide (CO2) from a surface if the surface coverage is 0.025 mol/m² and the temperature is 298 K. The enthalpy of adsorption for CO2 on the surface is -35.8 kJ/mol. The equilibrium constant (K) for the reaction is 2.99 x 10⁶ at 298 K.

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

0 votes

1 answer 64 views

Calculate the enthalpy change of isomerization for the conversion of n-butane to isobutane if the heat of combustion of n-butane is -2657.5 kJ/mol and the heat of combustion of isobutane is -2878.8 kJ/mol.

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

0 votes

1 answer 56 views

Calculate the equilibrium constant for the following electrochemical reaction at a temperature of 25°C:$$\ce{Co^{2+} + 2e^- <=> Co(s)}$$Given that the standard reduction potential for the half-reaction is $-0.28\,\text{V}$ and the concentration of $\ce{Co^{2+}}$ is $0.1\,\text{M}$.

asked Jan 23 in ElectroChemistry by Shawn33B4717 (1.9k points)

0 votes

1 answer 56 views

Calculate the equilibrium constant for a reaction involving a weak oxidizing agent where the concentration of the oxidizing agent is 0.1 M and the concentration of the reduced species is 0.05 M at equilibrium. The balanced chemical equation of the reaction is given as follows:OX + 2 e- ⇌ REDwhere OX is the weak oxidizing agent and RED is the reduced species.

asked Jan 23 in Chemical equilibrium by LeesaJ55672 (1.9k points)

0 votes

1 answer 102 views

A student has 20 grams of iron and 40 grams of oxygen. What is the limiting reactant in the reaction between iron and oxygen to form iron oxide (FeO)? How many grams of FeO can be produced assuming complete reaction and no excess reactants?

asked Jan 22 in Chemical reactions by CandelariaFe (1.6k points)

0 votes

1 answer 64 views

Calculate the enthalpy change of adsorption when 2.5 moles of nitrogen gas are adsorbed onto 10 g of activated charcoal at 298 K, given that the pressure of nitrogen gas is 1.0 atm. The molar mass of nitrogen is 28 g/mol, and the initial pressure of nitrogen is 0.5 atm.

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

0 votes

1 answer 113 views

A certain metal oxide has an enthalpy of formation of -589.3 kJ/mol. When a 5.60 g sample of this oxide is reduced with excess hydrogen gas, the enthalpy change for the reaction is found to be -129.3 kJ/mol. Calculate the enthalpy of reduction per mole of this oxide.

asked Jan 22 in ThermoChemistry by EnriquetaDam (2.3k points)

0 votes

1 answer 56 views

Calculate the equilibrium constant (Kc) for the reaction: 2A(g) + B(g) ⇌ C(g) + D(g), if the concentration of A is 0.25 M, the concentration of B is 0.10 M, the concentration of C is 0.30 M and the concentration of D is 0.20 M at equilibrium.

asked Jan 23 in Chemical thermodynamics by ElvaL9406057 (2.3k points)

0 votes

1 answer 54 views

Calculate the heat of hydration of copper (II) sulfate pentahydrate given that 5.00 g of the hydrate was dissolved in 100.0 mL of water at 25°C, and the resulting solution temperature increased from 25°C to 30°C. The molar mass of copper (II) sulfate pentahydrate is 249.685 g/mol and the specific heat capacity of water is 4.184 J/g°C.

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

0 votes

1 answer 54 views

Calculate the heat of hydration of 1 mole of anhydrous copper(II) sulfate (CuSO4) when it is dissolved in water to form its hydrated form, CuSO4·5H2O. Given the following information:- Heat of solution of anhydrous CuSO4: -74.9 kJ/mol- Enthalpy change of hydration of CuSO4·5H2O: -245.1 kJ/mol

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

0 votes

1 answer 65 views

Calculate the enthalpy change for the hydrolysis of 0.025 moles of ethyl acetate (C4H8O2) in the presence of excess water, given that the enthalpy of reaction is -56.0 kJ/mol.

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

0 votes

1 answer 65 views

Calculate the enthalpy change for the hydration of MgSO4 using the following data:MgSO4(s) → MgSO4(aq) ΔH1 = 44.5 kJ/molMgSO4(aq) + 7H2O(l) → MgSO4 • 7H2O(s) ΔH2 = -63.2 kJ/mol.

asked Jan 23 in ThermoChemistry by MistyReagan2 (1.4k points)

0 votes

1 answer 53 views

Calculate the lattice energy of MgO using Born-Haber Cycle. Given the following information: - The enthalpy change of sublimation of Mg = +1472 kJ/mol- The first ionization energy of Mg = +738 kJ/mol- The second ionization energy of Mg = +1450 kJ/mol- The enthalpy change of electron affinity of O = -141 kJ/mol- The enthalpy change of formation of MgO = -601 kJ/mol- Assume that all other enthalpy changes are negligible.

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

0 votes

1 answer 64 views

Calculate the enthalpy change for the reaction: 2H2(g) + O2(g) --> 2H2O(g) given the following enthalpy changes: H2(g) + 1/2O2(g) --> H2O(g) ΔH1 = -286 kJ/molH2(g) + 1/2Cl2(g) --> HCl(g) ΔH2 = -92 kJ/mol Cl2(g) --> 2Cl(g) ΔH3 = +242 kJ/molHCl(g) + 1/2O2(g) --> H2O(g) + Cl2(g) ΔH4 = -184 kJ/mol

asked Jan 23 in Chemical reactions by SheilaSchaef (1.8k points)

0 votes

1 answer 65 views

Calculate the enthalpy change for the following reaction, using Hess's Law:2H2S(g) + 3O2(g) → 2H2O(l) + 2SO2(g)Given the following enthalpy changes: 2H2(g) + O2(g) → 2H2O(l) ΔH1 = -484 kJ2SO2(g) + O2(g) → 2SO3(g) ΔH2 = -198 kJ2H2(g) + S(s) → H2S(g) ΔH3 = +25kJ

asked Jan 23 in Chemical reactions by BelenPickard (2.3k points)

0 votes

1 answer 56 views

Calculate the equilibrium constant (K) for the reaction that occurs when a nickel electrode is placed in a solution containing 1.0 M of nickel ions and 1.0 M of copper ions. The nickel electrode was placed in the solution, and the cell potential was measured to be 0.21 V at 25 °C.

asked Jan 23 in ElectroChemistry by CorneliusU11 (1.7k points)

0 votes

1 answer 67 views

Calculate the enthalpy change for the combustion of methane gas at standard conditions if 34.0 g of methane is burned completely in oxygen and releases 802 kJ of heat.

asked Jan 23 in ThermoChemistry by Dannie89E20 (2.0k points)

0 votes

1 answer 67 views

Calculate the enthalpy change for the combustion of methane gas (CH4) using Hess's Law, given the following equations and enthalpy changes: C(s) + O2(g) → CO2(g), ΔH = -393.5 kJ/mol2H2(g) + O2(g) → 2H2O(l), ΔH = -571.6 kJ/mol CH4(g) + 2O2(g) → CO2(g) + 2H2O(l), ΔH = ?

asked Jan 23 in ThermoChemistry by Alejandra79W (1.9k points)

0 votes

1 answer 54 views

Calculate the heat of crystallization, in kilojoules per mole, when 50.0 grams of sodium hydroxide (NaOH) is dissolved in 500.0 grams of water at 25⁰C and then cooled to 5⁰C, assuming that all the heat evolved during the process is transferred to the solution. The heat capacity of water is 4.18 J/gK, and the enthalpy of formation of NaOH is -425 kJ/mol.

asked Jan 23 in ThermoChemistry by OliverOtis4 (2.3k points)

Categories