Question

Part A Calculate the change in entropy that occurs in the system when 56.7 g of...

Part A Calculate the change in entropy that occurs in the system when 56.7 g of water vaporizes from a liquid to a gas at its boiling point (100.0?C). ?H?vap = 40.7 kJ/mol Express your answer to three significant figures.

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
Calculate the change in entropy that occurs in the system when 4.50 mol of diethyl ether...
Calculate the change in entropy that occurs in the system when 4.50 mol of diethyl ether (C4H10O) melts at its melting point (− 116.3 ∘C). ΔH∘fus=7.27kJ/mol . Express your answer in joules per kelvin to three significant figures.
Calculate the change in entropy of the surroundings when 1.0 mol of water vaporizes as 1000C....
Calculate the change in entropy of the surroundings when 1.0 mol of water vaporizes as 1000C. The heat of vaporization of water is 40.6 kj/mol
If the temperature of the surroundings is -244.32 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is -244.32 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 40.4 g of liquid oxygen (O2) freezes. Report your answers to two decimal places. Tfus(°C) -218.79 Tvap(°C) -182.96 ΔH°fus (kJ/mol) 0.44 ΔH°vap (kJ/mol) 6.82
For water ∆H°vap = 40.7 kJ/mol at 100.°C, its boiling point. Calculate w and ∆E for...
For water ∆H°vap = 40.7 kJ/mol at 100.°C, its boiling point. Calculate w and ∆E for the vaporization of 1.00 mol water at 100.°C and 1.00 atm pressure.
If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is 38.36 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 48.1 g of gaseous carbon tetrachloride (CCl4) condenses. Report your answers to two decimal places. Tfus(°C) -23.00 Tvap(°C) 76.80 ΔH°fus (kJ/mol) 3.28 ΔH°vap (kJ/mol) 29.82
Calculate the enthalpy change, ΔH, for the process in which 14.3 g of water is converted...
Calculate the enthalpy change, ΔH, for the process in which 14.3 g of water is converted from liquid at 4.0 ∘C to vapour at 25.0 ∘C . For water, ΔvapH = 44.0 kJ mol−1 at 25.0 ∘C and Cs = 4.18 J g−1 ∘C−1 for H2O(l). Express your answer to three significant figures and include the appropriate units.
If the temperature of the surroundings is 5.45 °C, calculate the entropy change (in J/K) for...
If the temperature of the surroundings is 5.45 °C, calculate the entropy change (in J/K) for the system (ΔSsys), surroundings (ΔSsur) and universe (ΔSuniverse) when 33.6 g of gaseous diethyl ether (C4H10O) condenses. Report your answers to two decimal places. Tfus(°C) -116.30 Tvap(°C) 34.50 ΔH°fus (kJ/mol) 7.27 ΔH°vap (kJ/mol) 26.52 i need these : 1- ΔSsys = 2- ΔSsur = 3 -ΔSuniverse =
Calculate the amount of heat ( in kJ) required to convert 344.0 g of liquid water...
Calculate the amount of heat ( in kJ) required to convert 344.0 g of liquid water at 22.5 oC into steam at 145.0 °C. ( Heat of vaporization of water at its boiling point = 40.7 kJ/mol., specific heats of water and steam are 4.184 J/g °C and 2.01 J/g °C, respectively. )
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...
Calculate the change in entropy of the system when 15.0g of ice at -12.0C is converted...
Calculate the change in entropy of the system when 15.0g of ice at -12.0C is converted to water vapor at 105C at a constant pressure of 1bar. The constant pressure molar heat capacity ofH2O (s) and H2O (l) is 75.291J/mol K and that of H2O (g) is 33.58 J/K mol
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT