Question

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 |

Answer #1

This is calculated in 3 steps.

1) To heat the ice from -36°C to 0°C (dT = 20°C)

Q = mcdT

Q = heat ,

m = mass of ice = 93 g

c = specific heat of ice = 2.09 J/g/°C

dT = temperature difference = 36°C

Q = 93 g x 2.09 J/g/°C x 36°C = 6997.32 J

Q = 6997.32 J

2) To melt the ice at 0°C
to water at 0°C.

Q = m x Enthalpy of fusion of water

= 93 g x 334 J/g

= 31062 J

Q = 31062 J

3) To heat the water from 0°C to boiling at 35°C

Q = mcdT where c = specific heat of water ,dT = 100°C

= 93 g x 4.18 J/g/°C x 35°C

= 13605.9 J

Q = 13605.9 J

Therefore,

Total amount of heat required = 6997.32 J + 31062 J + 13605.9 J

= 51665 J

= 52 kJ

Hence,

Ans = 52 kJ

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 ?

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)):...

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

Calculate the energy needed to heat 14.6 g ice
at -10.0 °C to liquid water at
70.0 °C. The heat of vaporization of water = 2257
J/g, the heat of fusion of water = 334 J/g, the specific heat
capacity of water = 4.18 J/g·°C, and the specific heat capacity of
ice = 2.06 J/g·°C.

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 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)

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
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What amount of thermal energy (in kJ) is required to convert 216
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melting point of water is 0 °C and its normal boiling point is 100
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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
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How much heat is required to convert solid ice with a mass of
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J/kgK, and the heat of fusion for water is Lf = 334
kJ/kg.
(in J)

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