Question

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: *s*ice=2.09 J/(g⋅∘C)

Specific heat of liquid water: *s*water=4.18 J/(g⋅∘C)

Enthalpy of fusion (H2O(s)→H2O(l)): Δ*H*fus=334 J/g

Enthalpy of vaporization (H2O(l)→H2O(g)): Δ*H*vap=2250
J/g

Answer #1

Ti = -18.0 oC

Tf = 25.0 oC

here

Cs = 2.09 J/g.oC

Heat required to convert solid from -18.0 oC to 0.0 oC

Q1 = m*Cs*(Tf-Ti)

= 46 g * 2.09 J/g.oC *(0--18) oC

= 1730.52 J

delta Hfusion = 334 J/g

Heat required to convert solid to liquid at 0.0 oC

Q2 = m*delta Hfusion

= 46.0g *334.0 J/g

= 15364 J

Cl = 4.18 J/g.oC

Heat required to convert liquid from 0.0 oC to 25.0 oC

Q3 = m*Cl*(Tf-Ti)

= 46 g * 4.18 J/g.oC *(25-0) oC

= 4807 J

Total heat required = Q1 + Q2 + Q3

= 1730.52 J + 15364 J + 4807 J

= 21901 J

= 21.9 KJ

Answer: 21.9 KJ

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

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 ?

How much heat energy, in kilojoules, is required to convert 48.0
g of ice at −18.0 ∘C to water at 25.0 ∘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 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.

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...

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)

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