Question

Calculate the amount of heat required to change 35.0g ice at -25.0 C to steam at 125 C (Heat of fusion = 333 J/g; heat of vaporization = 2260 J/g; Specific heats: ice = 2.09 J/g*K, water = 4.18 J/g*K, steam = 1.84 J/g*K)

Answer #1

Q = m c ∆T

Q = quantity of heat in joules (J)

m = mass of the substance acting as the environment in

grams (g)

c = specific heat capacity (4.19 for H2O) in J/(g
^{o}C)

∆T = change in temperature = Tfinal - Tinitial in ^{o}C

The "ICE" in this case is going to do 5 things:

a) as a solid, warm up from -25 to zero

b) all 35 g will melt

c) as a liquid, temperature reaches 100 Deg Cel

d) all 35 gm will convert to steam

e) as Steam it reaches temperature 125 Deg Cel

Q = 35 x 2.09 x 25 + 35 x 333 + 35 x 4.18 x 100 + 35 x 2260 + 35 x 1.84 x 125

Q = 1828.75 + 11655 + 14630 + 79100 + 8050

**Q = 115263.75 Joules or 115.263 Kilo joules of heat is
need to change 35.0g ice at -25.0 C to steam at
125C**

Calculate the amount of heat required to change 35.0 g ice at
-25.0ºC to steam at 125ºC. (Heat of fusion = 333 J/g; heat of
vaporization = 2260 J/g; specific heats: ice = 2.09 J/g·K, water =
4.18 J/g·K, steam = 1.84 J/g·K)

The enthalpy change for converting 10.0 g of ice at -25.0
degrees C to water at 80.0 degrees C is _______kJ. The
specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K,
and 1.84 J/g-K, respectively. For H2O, Delta Hfus=6.01
kJ/mol, and Delta Hvap=40.67 Kj/mol
Please explain steps used as well. Thank you.

Calculate the amount of heat energy required to
change 0.173 kg of ice at a temperature of -35 �C
to steam at a
temperature of 160 �C. (specific heat capacities
of ice, water and steam are 2090, 4180, 2010 J ⁄ kg ⁄
�C
respectively. Latent heat of fusion and vaporization of water
are
3.34e5, 2.26e6 J ⁄ kg respectively.)

part A How much heat energy, in
kilojoules, is required to convert 69.0 g of ice at −18.0 ∘C to
water at 25.0 ∘C ? Part B How long would it take
for 1.50 mol of water at 100.0 ∘C to be converted completely into
steam if heat were added at a constant rate of 22.0 J/s ?
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)):...

The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250 J/g
How much heat energy, in kilojoules, is required to convert 36.0
g of ice at −18.0 ∘C to water at 25.0 ∘C ?

To change 25 kg of ice -10°C to steam 100°C, how much heat is
required? The specific heat of water is 4.184 kJ/kg. K. The latent
heat of fusion for water at 0°C is approximately 334 kJ/kg (or 80
cal/g), and the latent heat of vaporization at 100°C is about 2,230
kJ/kg (533 cal/g).

11.
Consider the following specific heat capacities:
H2O (s) = 2.09 J/g·°C
H2O (l) = 4.18 J/g·°C
H2O (g) = 2.03 J/g·°C
The heat of fusion for water is 334 J/g and its heat of
vaporization is 2260 J/g. Calculate the amount of heat required to
convert 93 g of ice at -36°C completely to liquid water at
35°C.
52 kJ
21 kJ
7 kJ
38 kJ

What mass of steam at 100∘C must be added to 1.10 kg of ice at
0∘C to yield liquid water at 19 ∘C? The heat of fusion for water is
333 kJ/kg , the specific heat is 4186 J/kg⋅C∘ , the heat of
vaporization is 2260 kJ/kg .

How much heat energy, in kilojoules, is required to convert 46.0
g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to
three significant figures and include the appropriate units.
The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250
J/g

How much heat energy, in kilojoules, is required to convert 79.0
g of ice at −18.0 ∘C to water at 25.0 ∘C ? Express your answer to
three significant figures and include the appropriate units.
The constants for H2O are shown here:
Specific heat of ice: sice=2.09 J/(g⋅∘C)
Specific heat of liquid water: swater=4.18 J/(g⋅∘C)
Enthalpy of fusion (H2O(s)→H2O(l)): ΔHfus=334 J/g
Enthalpy of vaporization (H2O(l)→H2O(g)): ΔHvap=2250
J/g

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