Question

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 =

Homework Answers

Answer #1

We know condensation process is at equilibrium. So its delta G is zero. And so

Delta H = T delta S

We now delta H condensation and temperature. Lets put the number in.

Here Delta H condensation and we are given its delta H of vaporization.

Delta H vap = - delta Hcondensation

Therefore Delta H condensation = - 26.52 x 103 J /mol

Temperature at which condensation occur = 34.50 + 273.15 = 307.65 K

Delta Ssystem = - 26.52 E3 J /mol x 307.65 K= -8158878 J/K mol

We need entropy in J/K

Lets multiply it by number of moles of diethyl ether

Delta Ssystem = -8158878 x (33.6 g / 74.12 g mol-1)

= - 3698574 J/K

DeltaS of surrounding = - q / Tsurr , here surrounding temperature is 5.45 deg C

T = 5.45 + 273.15 = 278.6 k

Delta S surrounding = - 8158878 / 278.6 = 29285.3 J / K

Delta S universe Delta S system + Delta S surrounding = -3698574+29285.3=-3669289 J / K

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
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
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
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.
A) Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are...
A) Four ice cubes at exactly 0 ∘C with a total mass of 53.5 g are combined with 140 g of water at 85 ∘Cin an insulated container. (ΔH∘fus=6.02 kJ/mol, cwater=4.18J/g⋅∘C) If no heat is lost to the surroundings, what is the final temperature of the mixture? B) A sample of steam with a mass of 0.510 g and at a temperature of 100 ∘C condenses into an insulated container holding 4.50 g of water at 2.0 ∘C.( ΔH∘vap=40.7 kJ/mol,...
A sample of steam with a mass of 0.532 g at a temperature of 100 ∘C...
A sample of steam with a mass of 0.532 g at a temperature of 100 ∘C condenses into an insulated container holding 4.25 g of water at 4.0 ∘C. (For water, ΔH∘vap=40.7 kJ/mol and Cwater=4.18 J/(g⋅∘C).) Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?
A sample of steam with a mass of 0.520 g and at a temperature of 100...
A sample of steam with a mass of 0.520 g and at a temperature of 100 ∘C condenses into an insulated container holding 4.45 g of water at 5.0 ∘C.( ΔH∘vap=40.7 kJ/mol, Cwater=4.18 J/g⋅∘C) Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?
a. The standard enthalpy of vaporization of an inorganic compound is 38.9 kJ/mol. If the temperature...
a. The standard enthalpy of vaporization of an inorganic compound is 38.9 kJ/mol. If the temperature at which this phase change occurs is 221.72 °C, determine ΔS°vap (in J/mol/K) for this compound. Report your answer to three significant figures. b. The entropy of freezing of an organic compound is -21.0 J/mol/K. If ΔH°freez is -14.01 kJ/mol, determine the temperature (in K) at which this phase change occurs. Report your answer to two decimal places
Calculate ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for the following process at 298 K: HNO3(g) → HNO3(aq) HNO3(g)...
Calculate ΔS°(system), ΔS°(surroundings), and ΔS°(universe) for the following process at 298 K: HNO3(g) → HNO3(aq) HNO3(g) HNO3(aq) S°, J/K 266.38 146.4 ΔfH°, kJ/mol -135.06 -207.36 ΔS°(system) =  J/K∙mol ΔS°(surroundings) =  J/K∙mol ΔS°(universe) =  J/K∙mol
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of...
Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.25 kg of water decreased from 125 °C to 24.5 °C. Melting point: 0 degrees C Boiling Point: 100 degrees C Delta H(fus): 6.01 kJ/mol Delta H(vap): 40.67 kJ/mol cp(s): 37.1 J/mol x degrees C cp(l): 75.3 J/mol x degrees C cp(g): 33.6 J/mol x degrees C
15. The entropy change for a certain nonspontaneous reaction at 50 °C is 140 J/K. (a)...
15. The entropy change for a certain nonspontaneous reaction at 50 °C is 140 J/K. (a) Is the reaction endothermic or exothermic? (b) What is the minimum value of ΔH (in kJ) for the reaction? 16. What is the sign of ΔS in each of the following? (a) Freezing of water at 2 °C (b) Corrosion of iron metal (c) Expansion of a gas to fill the available volume (d) Separation of an unsaturated aqueous solution of potassium chloride into...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT