Question
In: Chemistry
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol, respectively, and the specific heat capacity of water is 4.18 J/g°C, calculate the total quantity of heat evolved when 27.1 g of steam at 216°C is condensed, cooled, and frozen to ice at -50.°C.
______KJ
Please show the steps
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
Given that the specific heat capacities of ice and steam are
2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and
vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol,
respectively, and the specific heat capacity of water is 4.18
J/g°C, calculate the total quantity of heat evolved when 20.4 g of
steam at 162°C is condensed, cooled, and frozen to ice at
-50.°C.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
Given that the specific heat capacities of ice and steam are
2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and
vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol,
respectively, and the specific heat capacity of water is 4.18
J/g°C, calculate the total quantity of heat evolved when 13.2 g of
steam at 192°C is condensed, cooled, and frozen to ice at
-50.°C.
Specific heat of ice: 2.09 J/(g⋅∘C Specific heat of liquid water: 4.18 J/(g⋅∘C) Enthalpy of fusion:...
Specific heat of ice: 2.09 J/(g⋅∘C
Specific heat of liquid water: 4.18 J/(g⋅∘C)
Enthalpy of fusion: ΔHfus=334J
Enthalpy of vaporization: ΔHvap=2250 J/g
How much heat energy, in kilojoules, is required to convert
47.0 g of ice at −−18.0 ∘C∘C to water at 25.0 ∘C?
Take the heat capacity of ice as 2.108 J/(g*C) and the heat capacity of water as...
Take the heat capacity of ice as 2.108 J/(g*C) and the heat
capacity of water as 4.184 J/(g*C) for this problem. For water,
DHfus = 6.001 kJ/mol at 0 C.
a. A 10.0 gram ice cube at -10.0 C is placed into 45.0 mL of
water at 40 C. Determine the final physical state and temperature
of the result. Calculate DS for the ice cube and the surrounding
water, and
Use the value DStot to explain why this process is...
The initial temperature of 140 g of ice is −22°C. The specific heat capacity of ice...
The initial temperature of 140 g of ice is −22°C. The specific
heat capacity of ice is 0.5 cal/g·C° and waters is 1 cal/g·C°. The
latent heat of fusion of water is 80 cal/g.
a. How much heat is required to raise the ice to 0°C?
b. How much additional heat is required to completely melt the
ice after it has reached 0°C?
c. How much additional heat is required to heat the water
(obtained by melting the ice) to...
How much heat is needed to convert 888 g of ice at -30°C to steam at...
How much heat is needed to convert 888 g of ice at -30°C to
steam at 136°C? (The specific heats of ice, steam, and liquid are
2.03 J/g · °C, 1.99 J/g · °C, and 4.18 J/g·°C, respectively. The
heat of fusion is 6.02 kJ/mol and heat of vaporization is 40.79
kJ/mol.)
________ kJ
How much heat is needed to convert 889 g of ice at -10°C to steam at...
How much heat is needed to convert 889 g of ice at -10°C to
steam at 136°C? (The specific heats of ice, steam, and liquid are
2.03 J/g·°C, 1.99 J/g·°C, and 4.18 J/g·°C, respectively. The heat
of fusion is 6.02 kJ/mol and heat of vaporization is 40.79 kJ/mol.)
kJ
How much heat is required to convert 84.9 g of ice at -17.0 C to steam...
How much heat is required to convert 84.9 g of ice at -17.0 C to
steam at 114 C?
1. Specific heat of water is 4.184 J/g ˚C. What is the heat in KJ gained...
1. Specific heat of water is 4.184 J/g ˚C. What is the heat in
KJ gained when 20 q of water is heated from 22˚C to 77˚C?
2. What is the heat in J to melt 100g of NaCl when the HF for
NaCl is 518 J/g?
3. What is the heat in J to equate 50 g Acetic Acid when the HE
= 390 J/g?
How much heat is released when 85.0 g of steam at 100.0°C is cooled to ice...
How much heat is released when 85.0 g of steam at 100.0°C is
cooled to ice at -15.0°C? The enthalpy of vaporization of water is
40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the
molar heat capacity of liquid water is 75.4 J/(mol ⋅ °C), and the
molar heat capacity of ice is 36.4 J/(mol ⋅ °C).
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