Question

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)

Answer #1

There are five steps:

1) Bring the ice from -25 C to 0 C.

Heat required per gram = C * Dt

=2.09 J/g·K x 25 K

= 52.25 J/g

2) Melt the ice:

Heat of fusion = 333 J/g

3) Bring the water from 0 to 100 C:

= C * Dt

=4.18 J/g·Kx 100K = 418 J/g

4) Vaporize the water:

heat of vaporization = 2260 J/g

5) Bring the steam from 100 to 125 C:

= C * Dt

1.84 J/g·K X25K

= 46 J/g

Total: 3109 J/g means this heat is require to change 1.0 g ice at
-25.0ºC to steam at 125ºC.

Now multiply it by 35.0 g and we get

=3109 J/g * 35.0 g

= **108815 J or 108.8 kJ** which is require to
change 35.0 g ice at -25.0ºC to steam at 125ºC.

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)

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)):...

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 amount of thermal energy (in kJ) is required to convert 220
g of ice at -18 °C completely to water vapour at 248 °C? The
melting point of water is 0 °C and its normal boiling point is 100
°C. The heat of fusion of water is 6.02 kJ mol-1 The heat of
vaporization of water at its normal boiling point is 40.7 kJ mol-1
The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific
heat...

What amount of thermal energy (in kJ) is required to convert 216
g of ice at -30 °C completely to water vapour at 198 °C? The
melting point of water is 0 °C and its normal boiling point is 100
°C. The heat of fusion of water is 6.02 kJ mol-1 The heat of
vaporization of water at its normal boiling point is 40.7 kJ mol-1
The specific heat capacity of ice is 2.09 J g-1 °C-1 The specific
heat...

The heat of combustion of bituminous coal is 2.50 × 10 4 J/g.
What quantity of the coal is required to produce the energy to
convert 27.0 kg of ice at 0.00°C to steam at 100.°C? specific heat
(ice) = 2.10 J/g°C specific heat (water) = 4.18 J/g°C heat of
fusion = 333 J/g heat of vaporization = 2258 J/g

Calculate the amount of heat ( in kJ) required to convert 344.0
g of liquid water at 22.5 oC into steam at 145.0
°C. ( Heat of vaporization of water at its boiling
point = 40.7 kJ/mol., specific heats of water and steam are 4.184
J/g °C and 2.01 J/g °C,
respectively. )

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.

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

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