Recent questions without an upvoted answer

0 votes

1 answer 40 views

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 IsaacGreig05 (450 points)

0 votes

1 answer 31 views

Calculate the standard enthalpy change for the dissolution of 3.00 moles of sodium chloride in water, given that the molar enthalpy of solution of sodium chloride is -3.88 kJ/mol.

asked Feb 3 in Chemical thermodynamics by FideliaG9436 (690 points)

0 votes

1 answer 22 views

Calculate the standard enthalpy change for the dissolution of 3 mol of potassium chloride (KCl) in 1000 mL of water, given that the molar enthalpy of dissolution is -17.4 kJ/mol.

asked Feb 3 in Chemical thermodynamics by CorinneMcwho (470 points)

0 votes

1 answer 26 views

Calculate the standard enthalpy change for the dissolution of 10 grams of potassium hydroxide (KOH) in 100 mL of water. Given that the molar enthalpy of dissolution of solid KOH is -57.61 kJ/mol and the density of water is 1 g/mL.

asked Feb 3 in Chemical thermodynamics by JKXJayme4881 (450 points)

0 votes

1 answer 35 views

Calculate the standard enthalpy change for the dissolution of 10 grams of NaCl in water at 25°C, given that the molar enthalpy of dissolution of NaCl is -3.9 kJ/mol.

asked Feb 3 in Chemical thermodynamics by CecilaL0378 (230 points)

0 votes

1 answer 41 views

Calculate the standard enthalpy change for the dissolution of 10 g of NaOH in 100 mL of water at 25°C if the molar enthalpy of dissolution is -44.5 kJ/mol.

asked Feb 3 in Chemical thermodynamics by ThereseRosso (310 points)

0 votes

1 answer 43 views

Calculate the standard enthalpy change for the complete combustion of methane gas (CH4) at 25°C and 1 atm pressure, given that the standard enthalpy of formation for CH4 is -74.9 kJ/mol and the standard enthalpy of formation for water (H2O) is -285.8 kJ/mol.

asked Feb 3 in Chemical thermodynamics by BettinaChirn (290 points)

0 votes

1 answer 30 views

Calculate the standard enthalpy change for the complete combustion of methane gas (CH4(g)) at constant pressure, given the balanced equation: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l). The standard enthalpies of formation of CO2(g), H2O(l), and CH4(g) are -393.5 kJ/mol, -285.8 kJ/mol, and -74.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by LachlanFrair (330 points)

0 votes

1 answer 31 views

Calculate the standard enthalpy change for the complete combustion of methane (CH4) at constant pressure and 298 K, given that the standard enthalpies of formation for CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by DebraAtkinso (230 points)

0 votes

1 answer 35 views

Calculate the standard enthalpy change for the complete combustion of 2 moles of methane gas under standard conditions, where all reactants and products are in their standard states. The balanced chemical equation for the combustion of methane is CH4(g) + 2O2(g) → CO2(g) + 2H2O(l), and the standard enthalpy of formation ΔH°f for methane, carbon dioxide, and water are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.

asked Feb 3 in Chemical thermodynamics by CecilB463053 (310 points)

0 votes

1 answer 33 views

Calculate the standard enthalpy change for the combustion reaction of octane (C8H18) using the following balanced chemical equation:C8H18 + 12.5O2 →8CO2 + 9H2O Given the standard enthalpies of formation for CO2, H2O, and octane are -394 kJ/mol, -286 kJ/mol, and -249 kJ/mol respectively.

asked Feb 3 in Chemical thermodynamics by MelvinSalomo (490 points)

0 votes

1 answer 44 views

Calculate the standard enthalpy change for the combustion of methane gas using the following reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g). Given the standard enthalpy of formation values for methane, carbon dioxide, and water, calculate the heat released or absorbed during this reaction. Express your answer in kJ/mol.

asked Feb 3 in Chemical thermodynamics by EmilieBobb0 (350 points)

0 votes

1 answer 28 views

Calculate the standard enthalpy change for the combustion of methane gas at standard conditions, given the following balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)Note: Standard conditions refer to a temperature of 25°C and a pressure of 1 atm.

asked Feb 3 in Chemical thermodynamics by GerardMaes99 (410 points)

0 votes

1 answer 38 views

Calculate the standard enthalpy change for the combustion of methane gas (CH4) given the balanced chemical equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)The relevant standard enthalpies of formation are:ΔHf°[CH4(g)] = -74.87 kJ/molΔHf°[CO2(g)] = -393.5 kJ/molΔHf°[H2O(l)] = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by EliBrinkman (370 points)

0 votes

1 answer 33 views

Calculate the standard enthalpy change for the combustion of methane (CH4) at constant pressure, given that the standard enthalpies of formation are -74.87 kJ/mol for methane and -393.51 kJ/mol for carbon dioxide (CO2), and 2H2(g) + O2(g) → 2H2O(l) has a standard enthalpy change of -571.66 kJ/mol.

asked Feb 3 in Chemical thermodynamics by KathrinPenne (350 points)

0 votes

1 answer 16 views

Calculate the standard enthalpy change for the combustion of ethene gas (C2H4(g)) to form carbon dioxide gas (CO2(g)) and water vapor (H2O(g)), given the following thermochemical equations: C2H4(g) + 3O2(g) → 2CO2(g) + 2H2O(g) ΔH°=-1411 kJ/mol2H2(g) + O2(g) → 2H2O(g) ΔH°=-484 kJ/mol

asked Feb 3 in Chemical thermodynamics by OpheliaTuggl (190 points)

0 votes

1 answer 34 views

Calculate the standard enthalpy change for the combustion of ethane (C2H6) given the balanced chemical equation:C2H6(g) + 3.5 O2(g) → 2CO2(g) + 3H2O(l)Assume all reactants and products are in standard states and use the following standard enthalpy of formation values:ΔHf°(C2H6) = -84.7 kJ/molΔHf°(CO2) = -393.5 kJ/molΔHf°(H2O) = -285.8 kJ/mol

asked Feb 3 in Chemical thermodynamics by RedaDoy9962 (310 points)

0 votes

1 answer 39 views

Calculate the standard enthalpy change for the combustion of ethane (C2H6) gas to form carbon dioxide (CO2) gas and water (H2O) vapor at 298 K and 1 atm. The balanced chemical equation for the reaction is: C2H6(g) + 3.5 O2(g) → 2 CO2(g) + 3H2O(g) Given that the standard enthalpy of formation for C2H6(g) is -84.68 kJ/mol, CO2(g) is -393.51 kJ/mol, and H2O(g) is -241.82 kJ/mol.

asked Feb 3 in Chemical thermodynamics by JennaFairfax (470 points)

0 votes

1 answer 30 views

Calculate the standard enthalpy change for the combustion of 1 mole of propane gas (C3H8) at standard conditions using the following balanced chemical equation: C3H8(g) + 5O2(g) -> 3CO2(g) + 4H2O(l)Given the standard enthalpy of formation values at 298K for C3H8(g), CO2(g), and H2O(l) as -103.8, -393.5, and -285.8 kJ/mol respectively, calculate the standard enthalpy change for the combustion reaction.

asked Feb 3 in Chemical thermodynamics by Margot259311 (930 points)

0 votes

1 answer 6 views

Calculate the standard enthalpy change for the combustion of 1 mole of methane gas (CH4) under standard conditions given the following balanced chemical equation:CH4(g) + 2O2(g)→CO2(g) + 2H2O(g)(Standard conditions: temperature of 298K and pressure of 1 bar)

asked Feb 3 in Chemical thermodynamics by MiriamOtis62 (690 points)

Recent questions without an upvoted answer

Categories