Recent questions in Chemical thermodynamics

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Calculate the enthalpy change for the combustion of methane gas (CH4) at standard conditions using the given relevant thermodynamic data:2H2(g) + O2(g) -> 2H2O(g); ΔH° = -483.7 kJ/molCH4(g) + 2O2(g) -> CO2(g) + 2H2O(g); ΔH° = ?

asked Jan 23 in Chemical thermodynamics by ValCurrier53 (390 points)

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Calculate the enthalpy change for the combustion of methane gas (CH4) at standard conditions given the following information: 4 moles of methane gas is burned in excess oxygen gas (O2) to form carbon dioxide gas (CO2) and liquid water (H2O). The enthalpy change for the combustion of 1 mole of methane gas is -890.4 kJ/mol.

asked Jan 23 in Chemical thermodynamics by RachaelBousq (390 points)

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

asked Jan 23 in Chemical thermodynamics by CharlotteBal (650 points)

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Calculate the enthalpy change for the combustion of 2 moles of methane gas (CH4) at constant pressure, given that the standard enthalpy of formation (ΔHf) of methane gas is -74.8 kJ/mol. Express your answer in kilojoules (kJ).

asked Jan 23 in Chemical thermodynamics by HarrisMcCask (270 points)

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Calculate the enthalpy change for the combustion of 1 mole of methane (CH4) gas given that the standard enthalpy of formation of methane is -74.8 kJ/mol, and the standard enthalpies of formation for carbon dioxide (CO2) and water (H2O) are -393.5 kJ/mol and -241.8 kJ/mol respectively. The balanced chemical equation for the reaction is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l)

asked Jan 23 in Chemical thermodynamics by CarriMxg5557 (390 points)

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Calculate the enthalpy change (in kJ/mol) for the chemical reaction: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) Given the standard enthalpies of formation (ΔHf°) for C2H5OH(l) = -277.6 kJ/mol, CO2(g) = -393.5 kJ/mol, and H2O(l) = -285.8 kJ/mol.

asked Jan 23 in Chemical thermodynamics by Breanna4436 (550 points)

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Calculate the change in Gibbs free energy for the reaction between hydrogen gas and iodine gas that forms hydrogen iodide gas. The balanced equation is as follows:H2(g) + I2(g) → 2HI(g)Assume a temperature of 298 K and use the following standard molar free energy of formation values:∆Gf° (HI) = -17.4 kJ/mol∆Gf° (H2) = 0 kJ/mol∆Gf° (I2) = 0 kJ/mol

asked Jan 23 in Chemical thermodynamics by KevinBrazeno (350 points)

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Calculate the change in entropy when 1 mole of methane gas (CH4) is burned completely in oxygen gas (O2) at constant pressure and 298 K.

asked Jan 23 in Chemical thermodynamics by MandyFinley (690 points)

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Calculate the change in entropy of the system when 2 moles of ammonia react to form 3 moles of hydrogen gas and 1 mole of nitrogen gas. The reaction takes place at a constant temperature of 298 K and at a pressure of 1 atm. The molar entropy of each component in the reaction is given below:Ammonia: 192.5 J/K·molHydrogen gas: 130.6 J/K·molNitrogen gas: 191.6 J/K·mol

asked Jan 23 in Chemical thermodynamics by AlisonEastwo (660 points)

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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 TressaV9423 (210 points)

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Calculate the change in entropy (ΔS) of the following reaction at 298 K:2SO2(g) + O2(g) → 2SO3(g) Given the standard molar entropies at 298 K: ΔS°(SO2,g) = 248.2 J/Kmol ΔS°(O2,g) = 205.0 J/Kmol ΔS°(SO3,g) = 256.2 J/Kmol

asked Jan 23 in Chemical thermodynamics by JacquieElias (390 points)

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Calculate the change in entropy (in J/K) for the following reaction at 298 K: 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) Given the following standard entropy values (in J/K): CH3OH (l): 126.6, O2 (g): 205.0, CO2 (g): 213.6, H2O (l): 69.9

asked Jan 23 in Chemical thermodynamics by DorieKyle916 (610 points)

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Calculate the amount of heat required to raise the temperature of 50 g of water from 25°C to 100°C, given the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in Chemical thermodynamics by LesleeShumak (500 points)

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A student wants to calculate the reaction quotient, Q, for the following chemical reaction at 298 K:2H2(g) + O2(g) ⇌ 2H2O(g)If the partial pressures of H2, O2, and H2O are 0.25 atm, 0.15 atm, and 0.1 atm, respectively, what is the value of Q?

asked Jan 22 in Chemical thermodynamics by WyattBaker3 (310 points)

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A chemistry student needs to calculate the standard enthalpy change for the combustion reaction of methane gas (CH4) at 298 K and 1 atm pressure. The equation for the reaction is:CH4(g) + 2O2(g) --> CO2(g) + 2H2O(l)Given the following standard enthalpies of formation at 298 K:ΔHf(CO2) = -393.5 kJ/molΔHf(H2O) = -285.8 kJ/molΔHf(CH4) = -74.8 kJ/molCalculate ΔHrxn, the standard enthalpy change for the combustion reaction of methane gas.

asked Jan 22 in Chemical thermodynamics by Rodrick46Q1 (350 points)

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A chemistry student needs to calculate the standard enthalpy change for the combustion reaction of methane (CH4) to produce carbon dioxide (CO2) and water (H2O) at 298 K. The student is given the following information: CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH°rxn = -890.4 kJ/molThe enthalpy of formation of CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively. Using this data, what is the standard enthalpy change for the combustion reaction of methane (CH4) to produce carbon dioxide (CO2) and water (H2O) at 298 K?

asked Jan 22 in Chemical thermodynamics by JeannetteBru (530 points)

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A 25 g sample of water at 25°C is heated by 200 J. The temperature of the water increases to 40°C. Calculate the specific heat capacity of water.

asked Jan 22 in Chemical thermodynamics by ThaliaEsmond (470 points)

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A 25 g sample of water at 25°C is heated by 200 J. The temperature of the water increases to 40°C. Calculate the specific heat capacity of water.

asked Jan 22 in Chemical thermodynamics by CherylYoul4 (370 points)

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