Question

There are 270 Calories in a Hershey's® Milk Chocolate bar. The following data might be useful:...

There are 270 Calories in a Hershey's® Milk Chocolate bar. The following data might be useful: ΔHvap = 43.9 kJ/mol, ΔHfusion = 6.02 kJ/mol, ΔHsublimation = 49.9 kJ/mol, specific heat of ice = 2.05 J g-1°C-1, specific heat of water = 4.18 J g-1°C-1, and specific heat of steam = 2.08 J g-1°C-1. Assume the specific heat of water does not change with temperature. (Density of ice = 0.920 g/mL).

How much energy is used up at each step of the heating, including heating the solid, melting, heating the liquid, and vaporization?

If all of the energy in the bar were used to heat up 75.0 mL of ice at -25.0 °C, how hot would the water get?

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A 485.4-g sample of an element at 192°C is dropped into an ice–water mixture; 117.0 g...
A 485.4-g sample of an element at 192°C is dropped into an ice–water mixture; 117.0 g of ice melts and an ice–water mixture remains. Calculate the specific heat of the element. ΔHfusion = 6.02 kJ/mol (for liquid water at 0°C). Specific heat =______ J/g∙°C
A 500.0-g sample of an element at 153°C is dropped into an ice-water mixture; 109.5-g of...
A 500.0-g sample of an element at 153°C is dropped into an ice-water mixture; 109.5-g of ice melts and an ice-water mixture remains. Calculate the specific heat of the element from the following data: Specific heat capacity of ice: 2.03 J/g-°C Specific heat capacity of water: 4.18 J/g-°C H2O (s) → H2O (l), ΔHfusion: 6.02 kJ/mol (at 0°C) a) If the molar heat capacity of the metal is 26.31 J/mol-°C, what is the molar mass of the metal, and what...
What quantity of energy does it take to convert 0.200 kg ice at –20.°C to steam...
What quantity of energy does it take to convert 0.200 kg ice at –20.°C to steam at 250.°C? Specific heat capacities: ice, 2.03 J/g·°C; liquid, 4.2 J/g·°C; steam, 2.0 J/g·°C; = 40.7 kJ/mol;  = 6.02 kJ/mol. What is the energy in kJ
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...
Calculate the amount of energy necessary to warm 10.0 g of ice from 0.0° C to...
Calculate the amount of energy necessary to warm 10.0 g of ice from 0.0° C to 137.0° C. Express your answer in kJ. Do not enter units of measurement, do not enter the answer in scientific notation. The specific heat is 4.184 J/g∙°C for water and 1.99 J/g∙°C for steam. ΔHvap is 40.79 kJ/mol and ΔHfus is 6.01 kJ/mol.
Which of the following would release the most heat? Assume the same mass of in each...
Which of the following would release the most heat? Assume the same mass of in each case. Specific heats of ice, liquid water, and water vapor are 2.05 J/(g⋅°C), 4.18 J/(g⋅°C), and 2.01 J/(g⋅°C) respectively, the heat of fusion of ice is 6.01 kJ/mol, the heat of vaporization of water is 40.7 kJ/mol. (Please show your work) a. Heating the H2) sample from –14°C to 58°C. b. Cooling the H2O sample from 18°C to –2.3°C. c. Cooling the sample from...
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...
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)):...
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...
Heat, q, is energy transferred between a system and its surroundings. For a process that involves...
Heat, q, is energy transferred between a system and its surroundings. For a process that involves a temperature change q=m?Cs??T where Cs is specific heat and m is mass. Heat can also be transferred at a constant temperature when there is a change in state. For a process that involves a phase change q=n??H where, n is the number of moles and ?H is the enthalpy of fusion, vaporization, or sublimation. The following table provides the specific heat and enthalpy...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT