Question

Calculate the energy needed to heat 14.6 g ice at -10.0 °C to liquid water at...

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.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Ti = -10.0

Tf = 70.0

here

Cs = 2.06 J/g.oC

Heat required to convert solid from -10.0 to 0.0

Q1 = m*Cs*(Tf-Ti)

= 14.6 g * 2.06 J/g.oC *(0-(-10)) oC

= 300.76 J

Lf = 334.0

Heat required to convert solid to liquid at 0.0

Q2 = m*Lf

= 14.6 g *334.0 J/g

= 4876.4 J

Cl = 4.18 J/g.oC

Heat required to convert liquid from 0.0 to 70.0

Q3 = m*Cl*(Tf-Ti)

= 14.6 g * 4.18 J/g.oC *(70-0) oC

= 4271.96 J

Total heat required = Q1 + Q2 + Q3

= 300.76J + 4876.4J + 4271.96 J

= 9449 J

= 9.45*10^3 J (Taking into account significant figure)

Answer: 9.45*10^3 J

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The enthaply of fusion of ice is 334 J/g. The heat capacity of liquid water is...
The enthaply of fusion of ice is 334 J/g. The heat capacity of liquid water is 4.18 j/gxC. What is the smallest number of ice cubes at 0C, each containing one mole of water necessary to cool 500 g of liquid water intially at 20 C to 0 C?
Calculate the amount of energy (in kJ) required to heat 10.0 g of water from 50.0°C...
Calculate the amount of energy (in kJ) required to heat 10.0 g of water from 50.0°C to 150.°C at constant pressure. (specific heat capacity of liquid water is 4.18 J/g⋅K; specific heat capacity of water vapor is 1.84 J/g⋅K; heat of vaporization of water is 2.260 kJ/g). (1) 16.2 kJ (2) 25.6 kJ (3) 5.4 kJ (4) 33.2 kJ (5) 1.6 kJ I know that the answer is (2) 25.6 KJ but I do not know how to get to...
The constants for H2O are shown here: Specific heat of ice: sice=2.09 J/(g⋅∘C) Specific heat of...
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 46.0 g of ice at −18.0...
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...
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...
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 energy (in kilojoules) is needed to heat 4.65 g of ice from -11.5 ∘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.
100. g of ice at 0 degrees C is added to 300.0 g of water at...
100. g of ice at 0 degrees C is added to 300.0 g of water at 60 degrees C. Assuming no transfer of heat to the surroundings, what is the temperature of the liquid water after all the ice has melted and equilibrium is reached? 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
What amount of thermal energy (in kJ) is required to convert 220 g of ice at...
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...
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...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT