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Recent questions in Chemistry
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Calculate the entropy change when one mole of helium gas is compressed isothermally at 298 K from a volume of 10 L to 2 L. The heat capacity of helium at constant pressure, Cₚ, is 20.8 J/mol*K.
asked
Jan 23
in
Physical Chemistry
by
ChanteStroh
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1.5k
points)
0
votes
1
answer
41
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Calculate the entropy change of the following reaction at 25°C and 1 atm pressure:2NH3(g) + 3Cl2(g) → N2(g) + 6HCl(g)Given the standard entropy values are:ΔS°NH3 = 192.5 J/K•molΔS°Cl2 = 223.1 J/K•molΔS°N2 = 191.6 J/K•molΔS°HCl = 186.9 J/K•mol
asked
Jan 23
in
Chemical thermodynamics
by
KatieManzi6
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1.6k
points)
0
votes
1
answer
61
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Calculate the entropy change of an ideal monatomic gas at 1 atm and 300 K when it expands isothermally to 5 times its initial volume.
asked
Jan 23
in
Physical Chemistry
by
Shawn33B4717
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1.9k
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votes
1
answer
64
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Calculate the entropy change for the reaction: 2H2(g) + O2(g) → 2H2O(g)given that the standard molar entropies of H2(g), O2(g), and H2O(g) are 130.7 J/mol.K, 205.0 J/mol.K, and 188.8 J/mol.K, respectively.
asked
Jan 23
in
Chemical thermodynamics
by
ZitaHarrell8
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1.8k
points)
0
votes
1
answer
62
views
Calculate the entropy change for the reaction of 2 moles of methane gas reacting with 4 moles of oxygen gas to form carbon dioxide gas and water vapor at a constant temperature of 298 K. The reaction is balanced and the standard entropy values for methane, oxygen, carbon dioxide, and water vapor are given as -0.242, 205.16, 213.74, and 188.72 J/K/mol, respectively.
asked
Jan 23
in
Chemical thermodynamics
by
JackQ7308746
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2.0k
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0
votes
1
answer
55
views
Calculate the entropy change for the following chemical reaction at 25 °C: 2H2(g) + O2(g) → 2H2O(l) Given that the standard molar entropy of H2(g), O2(g), and H2O(l) are 130.68 J/mol·K, 205.03 J/mol·K and 70.01 J/mol·K respectively.
asked
Jan 23
in
Chemical thermodynamics
by
CecileBills
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2.2k
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0
votes
1
answer
72
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Calculate the entropy change for the combustion of methane at a constant temperature and pressure of 298 K and 1 atm, respectively. The balanced equation for the reaction is:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l)
asked
Jan 23
in
Chemical thermodynamics
by
IsraelSeidel
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1.3k
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0
votes
1
answer
54
views
Calculate the entropy change for the combustion of methane (CH4) at 298 K and 1 atm pressure, given the standard molar entropies of CH4, H2O (g), and O2 (g) are 186.3 J/K/mol, 188.7 J/K/mol, and 205.0 J/K/mol, respectively. The balanced chemical equation for the reaction is:CH4 (g) + 2 O2 (g) -> CO2 (g) + 2 H2O (g)
asked
Jan 23
in
Chemical thermodynamics
by
BelenPickard
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2.3k
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0
votes
1
answer
51
views
Calculate the entropy change (ΔS) for the reaction below at 298 K:2H2(g) + O2(g) → 2H2O(l)Given the standard molar entropy values are:H2(g) = 130.68 J/K molO2(g) = 205.03 J/K molH2O(l) = 69.91 J/K mol
asked
Jan 23
in
Chemical thermodynamics
by
ChasityBelli
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2.2k
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0
votes
1
answer
76
views
Calculate the entropy change (ΔS) for the combustion of methane gas (CH4) at constant pressure and standard conditions, given the following data: C(s) + O2(g) → CO2(g) ΔS° = -394 J/K·mol 2H2(g) + O2(g) → 2H2O(l) ΔS° = -237 J/K·mol CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH° = -802 kJ/mol
asked
Jan 23
in
Chemical thermodynamics
by
MargueriteWa
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1.8k
points)
0
votes
1
answer
55
views
Calculate the entropy change (∆S) when a container of volume 1.0 L is filled with 1.0 mol of ideal gas at a temperature of 300 K and a pressure of 1.0 atm, and then the gas is allowed to expand irreversibly to fill a volume of 2.0 L against a constant external pressure of 0.5 atm at the same temperature.
asked
Jan 23
in
Physical Chemistry
by
ChloeBodnar
(
2.0k
points)
0
votes
1
answer
68
views
Calculate the entropy change (∆S) for the reaction of 2 moles of solid NH4Cl with 1 mole of NaOH in a coffee cup calorimeter at a constant temperature of 25°C. The reaction takes place in 100 mL of water and produces 2 moles of NH3 and 1 mole of NaCl in solution. Assume that the specific heat capacity of water is 4.18 J/g·K and that the final solution temperature after the reaction is complete is 25°C.
asked
Jan 23
in
Chemical thermodynamics
by
GlendaNester
(
1.8k
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0
votes
1
answer
55
views
Calculate the entropy change (∆S) for the reaction between 2.0 moles of hydrogen gas (H2) and 1.0 mole of oxygen gas (O2) at constant pressure and a temperature of 298 K, given the standard molar entropy values for H2 and O2 to be 130.7 J/K•mol and 205.0 J/K•mol, respectively.
asked
Jan 23
in
ThermoChemistry
by
RoderickKyle
(
2.4k
points)
0
votes
1
answer
62
views
Calculate the enthalpy of vaporization of water given the following information: - The boiling point of water is 100°C- The specific heat capacity of liquid water is 4.18 J/g·°C- The specific heat capacity of steam is 1.84 J/g·°C- The heat of fusion of water is 40.7 kJ/mol - The molar mass of water is 18.015 g/mol- The heat capacity of the container is negligible- Assume that the vaporized water behaves ideally and has a constant heat capacity
asked
Jan 23
in
ThermoChemistry
by
Latonya89F54
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2.2k
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0
votes
1
answer
50
views
Calculate the enthalpy of vaporization of water given that it has a vapor pressure of 1.00 atm at 100°C and its molar enthalpy of vaporization at 373 K is 40.7 kJ/mol.
asked
Jan 23
in
ThermoChemistry
by
MoniqueBrins
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1.9k
points)
0
votes
1
answer
54
views
Calculate the enthalpy of vaporization of water at a temperature of 100 degrees Celsius and a pressure of 1 atm, given that the boiling point of water is 100 degrees Celsius and its enthalpy of vaporization at standard conditions (100 degrees Celsius and 1 atm) is 40.7 kJ/mol.
asked
Jan 23
in
ThermoChemistry
by
SOYRyan09176
(
1.6k
points)
0
votes
1
answer
70
views
Calculate the enthalpy of vaporization for water if 50.0 g of water is completely vaporized at its boiling point (100°C) using 107 kJ/mol as the heat of vaporization of water.
asked
Jan 23
in
ThermoChemistry
by
EvieOconnor
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2.3k
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0
votes
1
answer
55
views
Calculate the enthalpy of vaporization for water given the following information: The boiling point of water is 100°C and its specific heat capacity is 4.18 J/g°C. The density of water at its boiling point is 0.958 g/mL and the heat of fusion for water is 40.7 kJ/mol. The molar mass of water is 18.015 g/mol.
asked
Jan 23
in
ThermoChemistry
by
KathiFatnown
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1.6k
points)
0
votes
1
answer
57
views
Calculate the enthalpy of vaporization for water at 100 °C, given that the vapor pressure of water is 101.325 kPa and its molar volume is 18.07 L/mol at boiling point.
asked
Jan 23
in
ThermoChemistry
by
Murray05Y450
(
1.9k
points)
0
votes
1
answer
54
views
Calculate the enthalpy of vaporization for propane given its heat of fusion is 0.513 kJ/mol and heat of vaporization is 15.90 kJ/mol. The molar mass of propane is 44.10 g/mol.
asked
Jan 23
in
ThermoChemistry
by
PalmaYuille
(
2.1k
points)
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