How much heat, in kilojoules, is released when a 67.35 g sample of cesium metal is cooled from 725 °C to 335 °C?
Potentially Useful Information for cesium:
| Melting Point (°C) | 28.5 |
| Boiling Point (°C) | 671 |
| s(s) (J/g·°C) | 0.242 |
| s(l) (J/g·°C) | 0.177 |
| s(g) (J/g·°C) | 0.157 |
| ΔH°fus (kJ/mol) | 2.087 |
| ΔH°vap (kJ/mol) | 74.4 |
Please show a heating curve diagram
How much heat, in kilojoules, is released when a 67.35 g sample of cesium metal is...
How much energy (in kilojoules) is released when 31.5 g of ethanol vapor at 97.0 ∘C is cooled to -13.5 ∘C? Ethanol has mp = -114.5 ∘C, bp = 78.4 ∘C, ΔHvap = 38.56 kJ/mol and ΔHfusion = 4.60 kJ/mol. The molar heat capacity is 113 J/(K⋅mol) for the liquid and 65.7 J/(K⋅mol) for the vapor.
Calculate the total amount of heat required to heat 10.0 g of CCl4 (m.p. = -22.6 °C, b.p. = 78.3 °C) from -30 °C to 100 °C, given the following information: C°p,s = 0.287 J/g°C, C°p,l = 0.854 J/g°C, C°p,g = 0.537 J/g°C, ΔH°fus = 2.56 kJ/mole, and ΔH°vap = 29.8 kJ/mole.
How much energy is required to freeze 91.7 g of acetone (molar mass=58.08 g/mol) at its melting point, if its ΔH fus = 7.27 kJ/mol?
How much energy (in kilojoules) is released when 12.6 g of steam at 110.5 ∘C is condensed to give liquid water at 67.0 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor.
How much energy (in kilojoules) is released when 13.9 g of steam at 112.0 ∘C is condensed to give liquid water at 69.5 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor.
Calculate the change in entropy that occurs in the system when 49.0 g of acetone (C3H6O) freezes at its melting point (-94.8∘C). ΔH∘fus = 5.69 kJ/mol. Answer in J/K
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how much heat is released when 10.0 g of steam (water vapor ) at 105.0 C is cooled to liquid water at 25 C? S(water) = 4.18 J/g.C. ... S(steam) = 2.01 j/ g.C the heat of fusion of water is 6.02 KJ/ mol. The heat of vaporization of water is 40.7 KJ/mol
1. How much energy (in kilojoules) is released when 16.4 g of steam at 116.5 ∘C is condensed to give liquid water at 60.5 ∘C? The heat of vaporization of liquid water is 40.67 kJ/mol, and the molar heat capacity is 75.3 J/(K⋅mol) for the liquid and 33.6 J/(K⋅mol) for the vapor. 2.What is the entropy of fusion, ΔSfusion [in J/(K⋅mol)] for sodium? The necessary data are the following: mp = 97.8 ∘C,bp = 883 ∘C, ΔHvap = 89.6kJ/mol, and...
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