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Recent questions in ThermoChemistry
0
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1
answer
52
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Calculate the heat of crystallization of 10 grams of sodium acetate trihydrate (NaC2H3O2•3H2O) when it is cooled from 50°C to 10°C and crystallizes. The specific heat capacity of water is 4.18 J/g°C. The molar mass of sodium acetate is 82.03 g/mol.
asked
Jan 23
in
ThermoChemistry
by
LaunaSanches
(
310
points)
0
votes
1
answer
42
views
Calculate the heat of crystallization in kJ/mol of a substance, given that 100 g of it dissolved in water and cooled from 60°C to 20°C, releasing 5490 J of heat. The molar mass of the substance is 120 g/mol.
asked
Jan 23
in
ThermoChemistry
by
CarmaDurden
(
280
points)
0
votes
1
answer
41
views
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
JimGullett4
(
310
points)
0
votes
1
answer
55
views
Calculate the heat of crystallization for NaCl from the given data:The enthalpy of fusion of NaCl = 28.3 kJ/mol and the heat capacity of NaCl is approximately constant at 40.0 J/mol.K for temperatures close to room temperature. The melting point of NaCl is 801 °C and the density of the solid NaCl is 2.16 g/cm³.
asked
Jan 23
in
ThermoChemistry
by
DarnellSauls
(
550
points)
0
votes
1
answer
37
views
Calculate the heat of crystallization (in kJ/mol) of NaOH if 25g of NaOH dissolves in 100g of water at 25°C and releases 4.75kJ of heat.
asked
Jan 23
in
ThermoChemistry
by
WilliamCorco
(
190
points)
0
votes
1
answer
50
views
Calculate the heat of combustion for propane gas, C3H8(g), if 12.5 grams of propane are completely burned in excess oxygen gas and the products of reaction are cooled from 700°C to 25°C. The heat capacities of the reactants and products are as follows: C3H8(g): cp = 44.10 J/K O2(g): cp = 29.38 J/K CO2(g): cp = 36.8 J/K H2O(g): cp = 33.6 J/K Assume that the heat capacities of the products and reactants are constant over the temperature range of the reaction and that the heat lost to the surroundings is negligible.
asked
Jan 23
in
ThermoChemistry
by
OliveLeggo5
(
290
points)
0
votes
1
answer
41
views
Calculate the heat of adsorption of hydrogen gas on a platinum surface given the initial temperature of the system is 298 K and the final temperature is 330 K. The mass of the platinum surface used is 5 grams, and the amount of hydrogen adsorbed is 0.01 moles. Assume the heat capacity of the system is constant at 25 J/K.
asked
Jan 23
in
ThermoChemistry
by
ValRocha1287
(
310
points)
0
votes
1
answer
56
views
Calculate the heat energy required to sublime 25 grams of dry ice (CO2) at -78.5 °C, given the heat of sublimation for CO2 is 573 kJ/mol.
asked
Jan 23
in
ThermoChemistry
by
ShaynaHyatt3
(
270
points)
0
votes
1
answer
33
views
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
WillWilber35
(
530
points)
0
votes
1
answer
54
views
Calculate the heat (in kJ/mol) evolved when 1 mole of hydrogen gas is adsorbed on a surface if the enthalpy of adsorption for hydrogen is -30 kJ/mol.
asked
Jan 23
in
ThermoChemistry
by
DwainArreola
(
350
points)
0
votes
1
answer
49
views
Calculate the final temperature when 25 grams of aluminum at 80°C is placed in 100 grams of water at 25°C. The specific heat capacity of aluminum is 0.90 J/g°C and the specific heat capacity of water is 4.18 J/g°C.
asked
Jan 23
in
ThermoChemistry
by
MohammadWitt
(
450
points)
0
votes
1
answer
44
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
BrandyGlasfu
(
370
points)
0
votes
1
answer
44
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
BernieceBarn
(
470
points)
0
votes
1
answer
41
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
ClariceMcQui
(
190
points)
0
votes
1
answer
47
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
BlondellMann
(
210
points)
0
votes
1
answer
49
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
FelipeRudnic
(
350
points)
0
votes
1
answer
44
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
JacelynBecer
(
490
points)
0
votes
1
answer
44
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
TammiCady63
(
370
points)
0
votes
1
answer
45
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
Mozelle44F33
(
450
points)
0
votes
1
answer
53
views
Calculate the enthalpy of solution of sodium hydroxide (NaOH) in water, given that the heat absorbed by the solution is 128.0 kJ/mol and the molar concentration of the solution is 0.1 M. Assume that the specific heat capacity of the solution is the same as that of water (4.18 J/g⋅K) and that the density of the solution is 1.00 g/mL.
asked
Jan 23
in
ThermoChemistry
by
BillBonds192
(
790
points)
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Recent questions in ThermoChemistry
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