Question

Part A How much heat energy, in kilojoules, is required to convert 56.0 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.

Answer #1

Sensible heat (CP): heat change due to Temperature difference

Latent heat (LH): Heat involved in changing phases (no change of T)

Then

Q1 = m*Cp ice * (Tf – T1)

Q2 = m*LH ice

Q3 = m*Cp wáter * (Tb – Tf)

**Note** that Tf = 0°C; Tb = 100°C, LH ice = 334 kJ/kg;
LH water = 2264.76 kJ/kg.

Cp ice = 2.01 J/g°C ; Cp water = 4.184 J/g°C; Cp vapor = 2.030 kJ/kg°C

Then

Q1 = **56***2.01 * (0 – **-18**)

Q2 = **56***334

Q3 = **56***4.184 * (25– 0)

QT = Q1+Q2+Q3 = 2026.08 + 18704+5857.6 = 26587.68 J = 26.58 kJ

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

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 ?

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)):...

A.) How much heat is required to convert 15.0 g of ice at -13.0
∘C to steam at 100.0∘C ? Express your answer using three
significant figures. (Joules)
B.)How much heat is required to convert 15.0 g of ice at -13.0
∘C to steam at 100.0∘C? Express your answer using three significant
figures. (kcal)

How many kilojoules of energy are needed to convert 99.5 g of
ice at -13.1 to water at 20.0°C? (The specific heat of ice at -13.1
is 2.01 J/g°C.)

How many kilojoules of energy are needed to convert 83.0 g of
ice at -13.7 to water at 24.4°C? (The specific heat of ice at -13.7
is 2.01 J/g°C.)

How much energy (in kilojoules) is needed to heat 4.65 g of ice
from -11.5 ∘C to 20.5 ∘C? The heat of fusion of water is
6.01kJ/mol, and the molar heat capacity is 36.6 J/(K⋅mol) for ice
and 75.3 J/(K⋅mol) for liquid water.

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 is required to convert 32.5 g of ethanol at 28 ∘C
to the vapor phase at 78 ∘C?
Express your answer using two significant figures.

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