Question

The enthalpy change for converting 10.0g of ice at -50.0 degrees C to water at 50.0...

The enthalpy change for converting 10.0g of ice at -50.0 degrees C to water at 50.0 degrees C is ______ kJ. The specific heats of ice, water, and steam are 2.09J/g-K, 4.18J/g-K, respectively. For H2O Hfus=6.01kJ/mol and deltaHvap=40.67 kJ/mol.
A)12.28
B)4.38
C)3138
D)6.47
E)9.15
Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

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 enthalpy change for converting 10.0 g of ice at -25.0 degrees C to water at...
The enthalpy change for converting 10.0 g of ice at -25.0 degrees C to water at 80.0 degrees C is _______kJ.  The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g-K, respectively.  For H2O, Delta Hfus=6.01 kJ/mol, and Delta Hvap=40.67 Kj/mol Please explain steps used as well. Thank you.
What is the change in enthalpy (∆H) when a 147g of ice at -23.7°C is heated...
What is the change in enthalpy (∆H) when a 147g of ice at -23.7°C is heated to a liquid at 66.5°C? The specific heats of ice, liquid water, and steam are 2.03, 4.18, and 1.84 J/g°C, respectively. For water, ∆Hvap = 40.67 kJ/mol and ∆Hfus = 6.01 kJ/mol.
A 1.000 kg block of ice at 0 °C is dropped into 1.354 kg of water...
A 1.000 kg block of ice at 0 °C is dropped into 1.354 kg of water that is 45 °C. What mass of ice melts? Specific heat of ice = 2.092 J/(g*K) Water = 4.184 J/(g*K)   Steam = 1.841 J/(g*K) Enthalpy of fusion = 6.008 kJ/mol Enthalpy of vaporization = 40.67 kJ/mol
Please show each step. Thank you. How much heat (in kJ) is evolved in converting 1.00...
Please show each step. Thank you. How much heat (in kJ) is evolved in converting 1.00 mole of steam at 145.0 °C to ice at -50.0 °C? The heat capacity of ice is 2.09 J/g°C and that of steam is 2.09 J/g°C Heat of fusion for water • Hfus = 6.02 kJ/mol  Heat of vaporization for water • Hvap = 40.7 kJ/mol
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 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...
How much heat is released when 105 g of steam at 100.0°C is cooled to ice...
How much heat is released when 105 g of steam at 100.0°C is cooled to ice at -15.0°C? The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol • °C), and the molar heat capacity of ice is 36.4 J/(mol • °C).
Calculate the amount of energy in kilojoules needed to change 207 g of water ice at...
Calculate the amount of energy in kilojoules needed to change 207 g of water ice at −10 ∘C to steam at 125 ∘C. The following constants may be useful: Cm (ice)=36.57 J/(mol⋅∘C) Cm (water)=75.40 J/(mol⋅∘C) Cm (steam)=36.04 J/(mol⋅∘C) ΔHfus=+6.01 kJ/mol ΔHvap=+40.67 kJ/mol
Calculate the amount of energy in kilojoules needed to change 405 g of water ice at...
Calculate the amount of energy in kilojoules needed to change 405 g of water ice at −10 ∘C to steam at 125 ∘C. The following constants may be useful: Cm (ice)=36.57 J/(mol⋅∘C) Cm (water)=75.40 J/(mol⋅∘C) Cm (steam)=36.04 J/(mol⋅∘C) ΔHfus=+6.01 kJ/mol ΔHvap=+40.67 kJ/mol
Calculate the amount of energy in kilojoules needed to change 225 g of water ice at...
Calculate the amount of energy in kilojoules needed to change 225 g of water ice at −10 ∘C to steam at 125 ∘C. The following constants may be useful: Cm (ice)=36.57 J/(mol⋅∘C) Cm (water)=75.40 J/(mol⋅∘C) Cm (steam)=36.04 J/(mol⋅∘C) ΔHfus=+6.01 kJ/mol ΔHvap=+40.67 kJ/mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT