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Calculate the change in entropy for the combustion of methane gas (CH4) at constant pressure and temperature of 298 K. The products of the reaction are carbon dioxide gas (CO2) and water vapor (H2O). The molar entropy of CH4, CO2 and H2O at 298 K are 186.3 J/K/mol, 213.7 J/K/mol, and 188.8 J/K/mol, respectively.

asked Jan 23 in Chemical thermodynamics by TaylaBromby8 (2.2k points)

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Calculate the equilibrium constant (Kc) at 298 K for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g) given that the equilibrium concentration of NH3 is 0.20 M, N2 is 0.025 M, and H2 is 0.060 M.

asked Jan 23 in Chemical thermodynamics by StuartCarson (2.4k points)

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Calculate the amount of heat required to melt 20 grams of ice at 0°C and convert it to liquid water at 0°C. The enthalpy of fusion of water is 6.01 kJ/mol. Show all the steps of your calculations.

asked Jan 23 in ThermoChemistry by NilaBody107 (1.7k points)

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Calculate the heat of formation of Methane (CH4), given the following enthalpy changes:- Enthalpy change of combustion of methane = -890.4 kJ mol^-1- Enthalpy change of formation of water = -285.8 kJ mol^-1- Enthalpy change of formation of carbon dioxide = -393.5 kJ mol^-1

asked Jan 23 in Chemical bonding by ClydeC545764 (2.2k points)

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Calculate the change in enthalpy (ΔH) for the combustion of methane gas (CH4) at 25°C and constant pressure of 1 atm. The equation for the combustion of methane is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) Given the standard enthalpies of formation at 25°C are:ΔHf[CH4 (g)] = -74.87 kJ/mol ΔHf[CO2 (g)] = -393.5 kJ/mol ΔHf[H2O (l)] = -285.8 kJ/mol Assume that water is in its liquid phase at the end of the reaction.

asked Jan 23 in Physical Chemistry by RobertoLafla (2.1k points)

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A chemistry student wants to determine the effect of adding a buffer solution on the equilibrium position of an acetic acid-sodium acetate reaction. The initial concentrations of acetic acid and sodium acetate are both 0.1 M and the pH of the solution is 4. Calculate the new concentrations of acetic acid, acetate ion, and hydrogen ion after adding a buffer solution containing 0.2 M acetic acid and 0.2 M sodium acetate. What is the new pH of the solution?

asked Jan 22 in Chemical equilibrium by WPOBernadine (1.9k points)

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A student measures the current in a galvanic cell with a standard potential of 1.10 V, using a Zinc electrode and a Copper electrode. The student recorded the current as 0.50 A. What is the rate of the electrochemical reaction occurring in the cell?

asked Jan 22 in ElectroChemistry by LawrenceMcGr (1.8k points)

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Calculate the heat of crystallization for the solidification of 25 grams of a solution containing 10% sucrose (C12H22O11) by mass. The enthalpy of solution for sucrose in water at a given temperature is -5.73 kJ/mol. The molar mass of sucrose is 342.3 g/mol. Assuming that the solution completely solidifies upon cooling, determine the energy released or absorbed in the process.

asked Jan 23 in ThermoChemistry by BrandieB8434 (2.2k points)

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Calculate the enthalpy change for the isomerization reaction of butene-1 to cis-2-butene. Given that the standard enthalpy of formation for butene-1 is -19.8 kJ/mol and for cis-2-butene is -20.4 kJ/mol, and the standard enthalpy of combustion for butene-1 is -2876 kJ/mol.

asked Jan 23 in ThermoChemistry by TysonNettles (1.5k points)

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Calculate the enthalpy change of mixing 50 mL of 1 M HCl with 50 mL of 1 M NaOH at 25°C. It is known that the standard enthalpies of formation of HCl and NaOH are -92.3 kJ/mol and -469.2 kJ/mol, respectively. Assume that the heat capacity of the mixture is 4.18 J/g°C and the density of the solution is 1 g/mL.

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

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Calculate the enthalpy change for the isomerization of n-butane to iso-butane if the standard enthalpy of formation for n-butane is -125.7 kJ/mol and that for iso-butane is -147.4 kJ/mol. The isomerization reaction occurs at a constant pressure of 1 atm and at a temperature of 298 K.

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

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Calculate the boiling point of potassium chloride (KCl) using the Clausius-Clapeyron equation, given that its enthalpy of vaporization is 40.0 kJ/mol and its standard boiling point is 1500 K. What would be the expected boiling point of KCl at an atmospheric pressure of 1.0 atm (760 mmHg)?

asked Jan 23 in Inorganic Chemistry by ClevelandHaw (2.4k points)

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Calculate the heat absorbed or released during the crystallization of 50g of sodium acetate from a solution if the enthalpy change of the process is -3.9 kJ/mol.

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

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1 answer 52 views

Calculate the enthalpy of combustion for sucrose (C₁₂H₂₂O₁₁) given that 5.25 g of sucrose were burned in a bomb calorimeter and the temperature rose by 2.75 °C. The heat capacity of the calorimeter is 20.45 kJ/°C.

asked Jan 23 in ThermoChemistry by IWHJaxon1452 (2.1k points)

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1 answer 53 views

Calculate the enthalpy change of dissolution (in kJ/mol) for NaCl in water, given that 1.00 g of NaCl is dissolved in 50.0 mL of water at 25°C. The density of water is 0.997 g/mL and the specific heat capacity of the solution is assumed to be the same as that of water (4.184 J/gK). The molar mass of NaCl is 58.44 g/mol.

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

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Calculate the enthalpy of adsorption when 2.0 grams of activated charcoal adsorbs 25 mL of methane gas at a constant temperature of 298 K, given that the pressure is 1 atm. Assume ideal gas behavior for methane.

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

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Calculate the enthalpy change of desorption for a solid substance using the given data: The mass of the substance is 2.5 g, and the temperature change during desorption is 25 °C. The heat capacity of the substance is 1.5 J/g·°C. The molar mass of the substance is 150 g/mol. Assume that the desorption process takes place at constant pressure.

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

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Calculate the concentration of Cu2+ ions in a 0.1 M CuSO4 solution using the given standard reduction potential of Cu2+/Cu electrode and the measured cell potential. The electrode potential of the cell is 0.78 V and temperature is 25°C.

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

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Calculate the bond length between two hydrogen atoms that are covalently bonded together. Given that the distance between their nuclei is 74 pm and assume the bond is a perfect covalent bond with no ionic character.

asked Jan 23 in Chemical bonding by ScarlettRobb (1.7k points)

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Calculate the anodic Tafel slope for the following electrochemical reaction taking place at a platinum electrode:Fe2+(aq) + 2e- → Fe(s) Given that the exchange current density is 4.50 x 10^-4 A/cm^2 and the reaction rate constant for the reaction is 2.5 x 10^5 cm/s.

asked Jan 23 in ElectroChemistry by DeanI7567799 (2.2k points)

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