Question

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 ?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Ti = -18.0

Tf = 25.0

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)

= 36 g * 2.09 J/g.oC *(0--18) oC

= 1354.32 J

Lf = 334.0 J/g

Heat required to convert solid to liquid at 0.0 oC

Q2 = m*Lf

= 36.0g *334.0 J/g

= 12024 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)

= 36 g * 4.18 J/g.oC *(25-0) oC

= 3762 J

Total heat required = Q1 + Q2 + Q3

= 1354.32 J + 12024 J + 3762 J

= 17140 J

= 17.1 KJ

Answer: 17.1 KJ

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
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)):...
11. Consider the following specific heat capacities: H2O (s) = 2.09 J/g·°C H2O (l) = 4.18...
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
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.
Calculate the amount of heat required to change 35.0g ice at -25.0 C to steam at...
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 enthalpy change, ΔH, for the process in which 10.3 g of water is converted...
Calculate the enthalpy change, ΔH, for the process in which 10.3 g of water is converted from liquid at 9.4 ∘C to vapor at 25.0 ∘C . For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and Cs = 4.18  J/(g⋅∘C) for H2O(l). How many grams of ice at -24.5 ∘C can be completely converted to liquid at 9.8 ∘C if the available heat for this process is 5.03×103 kJ ? For ice, use a specific heat of 2.01 J/(g⋅∘C) and...
Part A Calculate the enthalpy change, ΔH, for the process in which 44.0 g of water...
Part A Calculate the enthalpy change, ΔH, for the process in which 44.0 g of water is converted from liquid at 7.6 ∘C to vapor at 25.0 ∘C . For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and s = 4.18 J/(g⋅∘C) for H2O(l) Express your answer numerically in kilojoules. Part B How many grams of ice at -11.0 ∘C can be completely converted to liquid at 9.4 ∘C if the available heat for this process is 5.66×103 kJ...
Part A) Calculate the enthalpy change, ΔH, for the process in which 38.6 g of water...
Part A) Calculate the enthalpy change, ΔH, for the process in which 38.6 g of water is converted from liquid at 0.3 ∘C to vapor at 25.0 ∘C . For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and Cs = 4.18  J/(g⋅∘C) for H2O(l). Part B) How many grams of ice at -24.6 ∘C can be completely converted to liquid at 9.4 ∘C if the available heat for this process is 4.04×103 kJ ? For ice, use a specific heat...
Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257...
Quantity per gram per mole Enthalpy of fusion 333.6 J/g 6010. J/mol Enthalpy of vaporization 2257 J/g 40660 J/mol Specific heat of solid H2O (ice) 2.087 J/(g·°C) * 37.60 J/(mol·°C) * Specific heat of liquid H2O (water) 4.184 J/(g·°C) * 75.37 J/(mol·°C) * Specific heat of gaseous H2O (steam) 2.000 J/(g·°C) * 36.03 J/(mol·°C) * At 1 atm, how much energy is required to heat 49.0 g of H2O(s) at − 18.0 °C to H2O(g) at 135.0 °C? Heat transfer...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT