Question

How many grams of ice at -5.3 ∘C can be completely converted to liquid at 28.8...

How many grams of ice at -5.3 ∘C can be completely converted to liquid at 28.8 ∘C if the available heat for this process is 5.30×103 kJ ? For ice, use a specific heat of 2.01 J/(g⋅∘C) and ΔHfus=6.01kJ/mol.

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
How many grams of ice at -23.5 ∘C can be completely converted to liquid at 28.9...
How many grams of ice at -23.5 ∘C can be completely converted to liquid at 28.9 ∘C if the available heat for this process is 5.63×103 kJ ? For ice, use a specific heat of 2.01 J/(g⋅∘C) and ΔHfus=6.01kJ/mol. Express your answer to three significant figures and include the appropriate units.
How many grams of ice at -22.6 ∘C can be completely converted to liquid at 29.9...
How many grams of ice at -22.6 ∘C can be completely converted to liquid at 29.9 ∘C if the available heat for this process is 5.47×103 kJ ? For ice, use a specific heat of 2.01 J g−1 ∘C−1 and ΔfusH=6.01kJ mol−1.
1. How many grams of ice at -6.9 ∘C can be completely converted to liquid at...
1. How many grams of ice at -6.9 ∘C can be completely converted to liquid at 28.4 ∘C if the available heat for this process is 4.59×103 kJ ? For ice, use a specific heat of 2.01 J/(g⋅∘C) and ΔHfus=6.01kJ/mol . Express your answer to three significant figures and include the appropriate units. 2. Now consider the following set of reactions: N2 + 2O2→N2O4 ,ΔH=−8 kJ/mol N2 + O2→2NO ,ΔH=180 kJ/mol What is the enthalpy for the following reaction? overall:...
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...
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...
How many grams of ice at -13°C must be added to 714 grams of water that...
How many grams of ice at -13°C must be added to 714 grams of water that is initially at a temperature of 83°C to produce water at a final temperature of 11°C. Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg·C° and of ice is 2050 J/kg·C°. For water the normal melting point is 0.00°C and the heat of fusion is 334 × 103...
How many grams of ice at -14°C must be added to 710 grams of water that...
How many grams of ice at -14°C must be added to 710 grams of water that is initially at a temperature of 81°C to produce water at a final temperature of 12°C. Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg·C° and of ice is 2050 J/kg·C°. For water the normal melting point is 0.00°C and the heat of fusion is 334 × 103...
How many grams of ice at -13°C must be added to 711 grams of water that...
How many grams of ice at -13°C must be added to 711 grams of water that is initially at a temperature of 87°C to produce water at a final temperature of 10°C? Assume that no heat is lost to the surroundings and that the container has negligible mass. The specific heat of liquid water is 4190 J/kg • C° and of ice is 2100 J/kg • C°. For water the normal melting point is 0.00°C and the heat of fusion...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT