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Calculate the standard enthalpy change for the vaporization of 25 grams of water at 100 degrees Celsius and 1 atmosphere of pressure, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
NorineFelici
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1.8k
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0
votes
1
answer
70
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Calculate the standard enthalpy change for the vaporization of 25 g of liquid nitrogen at its boiling point assuming constant pressure is 1 atm. Given the molar heat of vaporization of nitrogen is 5.56 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
OnitaLoftus1
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2.3k
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0
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1
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50
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Calculate the standard enthalpy change for the vaporization of 15 grams of water given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
LSCJoey08837
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2.2k
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1
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49
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Calculate the standard enthalpy change for the vaporization of 15 grams of water at its boiling point, given that the molar enthalpy of vaporization of water is 40.7 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
AudreaV25265
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2.0k
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0
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1
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67
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Calculate the standard enthalpy change for the vaporization of 100 g of water at 100°C given that the enthalpy of vaporization of water is 40.7 kJ/mol.
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Feb 3
in
Chemical thermodynamics
by
PDQJenifer7
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2.0k
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0
votes
1
answer
57
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Calculate the standard enthalpy change for the vaporization of 10 grams of water at 100°C, given that the enthalpy of vaporization for water is 40.7 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
LeathaOchoa
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1.7k
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0
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1
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41
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Calculate the standard enthalpy change for the vaporization of 1 mole of water at 100°C, given that the enthalpy of fusion of water is 6.01 kJ/mol and the enthalpy of vaporization of water is 40.7 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
CandraIdk507
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2.4k
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0
votes
1
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13
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Calculate the standard enthalpy change for the vaporization of 1 mole of water at 100°C and 1 atm pressure. The enthalpy of formation of liquid water is -285.8 kJ/mol and the enthalpy of formation of water vapor is -241.8 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
DoraSturm903
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1.8k
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0
votes
1
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70
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Calculate the standard enthalpy change for the transition of liquid water at 100°C to steam at the same temperature, given that the enthalpy of vaporization of water is 40.7 kJ mol-1.
asked
Feb 3
in
Chemical thermodynamics
by
MellisaOlivo
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1.9k
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0
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1
answer
51
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Calculate the standard enthalpy change for the sublimation of iodine, given that the sublimation of 1 mole of iodine requires 62.44 kJ of energy and the standard enthalpy of formation of iodine (s) is 0 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
MammieArmyta
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1.8k
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0
votes
1
answer
58
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Calculate the standard enthalpy change for the sublimation of iodine solid to iodine gas at 298 K with the following given data: - Standard enthalpy of fusion of iodine: 15.52 kJ/mol- Standard molar entropy of iodine solid: 62.7 J/K/mol- Standard molar entropy of iodine gas: 260.6 J/K/mol
asked
Feb 3
in
Chemical thermodynamics
by
ArlenBieber1
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1.9k
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0
votes
1
answer
54
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Calculate the standard enthalpy change for the sublimation of iodine at 25°C, given that the standard enthalpy of fusion of iodine is 15.7 kJ/mol and the standard enthalpy of vaporization of iodine is 41.0 kJ/mol. (The molar mass of iodine is 126.90 g/mol)
asked
Feb 3
in
Chemical thermodynamics
by
BYUBlake479
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2.0k
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0
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1
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43
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Calculate the standard enthalpy change for the sublimation of iodine (I2) using the given information: The standard enthalpy of fusion of iodine is 15.52 kJ/mol and the standard enthalpy of vaporization of iodine is 41.57 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
GracieGainfo
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2.2k
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0
votes
1
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37
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Calculate the standard enthalpy change for the sublimation of iodine (I2) if 1 mole of I2(s) is converted to 1 mole of I2(g) at 25°C and 1 bar pressure. Given the following information:- The standard enthalpy of fusion of I2 is 15.4 kJ/mol- The standard enthalpy of vaporization of I2 is 41.3 kJ/mol- The standard entropy change for the sublimation of I2 is 62.4 J/mol K.
asked
Feb 3
in
Chemical thermodynamics
by
Latonya89F54
(
2.2k
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0
votes
1
answer
60
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Calculate the standard enthalpy change for the sublimation of iodine (I2) given that the enthalpy of fusion for iodine is 15.52 kJ/mol and the enthalpy of vaporization for iodine is 41.57 kJ/mol.
asked
Feb 3
in
Chemical thermodynamics
by
DomenicAsbur
(
2.1k
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0
votes
1
answer
50
views
Calculate the standard enthalpy change for the sublimation of 5 moles of solid iodine (I2) given the following data:- Enthalpy of fusion of iodine = 15.52 kJ/mol- Enthalpy of vaporization of iodine = 41.57 kJ/mol
asked
Feb 3
in
Chemical thermodynamics
by
MaybellHoffm
(
2.2k
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0
votes
1
answer
58
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Calculate the standard enthalpy change for the reduction of iron(III) oxide to iron using the following balanced chemical equation:Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)Given that the standard enthalpy change of formation for Fe2O3(s) is -824.2 kJ/mol, the standard enthalpy change of formation for CO2(g) is -393.5 kJ/mol, and the standard enthalpy change of formation for Fe(s) is 0 kJ/mol. Assume all reactants and products are in their standard states.
asked
Feb 3
in
ThermoChemistry
by
BeatrisSanfo
(
1.7k
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0
votes
1
answer
58
views
Calculate the standard enthalpy change for the reduction of iron (III) oxide using carbon monoxide as the reducing agent, given that the standard enthalpy of formation for iron (III) oxide is -824.2 kJ/mol and the standard enthalpy of formation for carbon monoxide is -110.5 kJ/mol.
asked
Feb 3
in
ThermoChemistry
by
QTHGenevieve
(
1.7k
points)
0
votes
1
answer
59
views
Calculate the standard enthalpy change for the reaction:Cu(H2O)62+ (aq) + 4Cl-(aq) → CuCl42- (aq) + 12H2O (l)given the following standard enthalpies of formation:Cu(H2O)62+ (aq): -1846.4 kJ/molCuCl42- (aq): -3599.5 kJ/molH2O (l): -285.8 kJ/molCl- (aq): -167.2 kJ/mol
asked
Feb 3
in
Chemical thermodynamics
by
YaniraRhh59
(
1.9k
points)
0
votes
1
answer
55
views
Calculate the standard enthalpy change for the reaction: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) given the following enthalpy changes: ∆Hf° for NaCl(aq) = -407.3 kJ/mol ∆Hf° for H2O(l) = -285.8 kJ/mol ∆Hf° for NaOH(aq) = -469.11 kJ/mol ∆Hf° for HCl(aq) = -167.16 kJ/mol
asked
Feb 3
in
Chemical thermodynamics
by
KreogMoore5
(
6.4k
points)
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