What is the entropy change in J/K to the universe when a dry ice (CO2) sculpture...

Question

Question

Answer 1

Answer #1

Answer- dS_univ 0.331 kJ/K

Mass of CO₂ = 386.1 g

Molar mass of CO₂ = 44 g/mol

Moles of CO₂ = 389/MW = 386.1/44 = 8.775

heat required for sublimation of 1 mol of solid CO₂= 21.6 kJ/mol

So, heat required for sublimation of 8.775 moles of solid CO₂ = 8.775×21.6 = 189.54 kJ

dS_univ = dS_sys + dS_surr

Using relation:

dS = q/T

dS_sys = 189.54/(273-78.5) = 0.974 kJ/K

dS_surr = -189.54/(273+21.7) = -0.643 kJ/K

So,

dS_univ = 0.974 - 0.643 = 0.331 kJ/K

Your one thumbs up will help me lot. Thanks!

Add a comment

Answer 2

Similar Homework Help Questions

17.34. Another decorative "ice" sculpture is carved from dry ice (solid CO2) and held at its...

17.34. Another decorative "ice" sculpture is carved from dry ice (solid CO2) and held at its sublimation point of -78.5 C. What is the entropy change to the universe when the COp sculpture, weighing 389 g, sublimes on a granite tabletop if the temperature of the granite is 12'C and the process occurs reversibly? Assume a final temperature for the CO vapor of -78.5 C. The heat of sublimation of CO2 is 26.1 kJ/mol.
PartA Calculate the amount of heat required to completely sublime 97.0 g of solid dry ice...

PartA Calculate the amount of heat required to completely sublime 97.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJ/mol. Part B How much heat is evolved in converting 1.00 mol of steam at 155.0 ∘C to ice at -55.0 ∘C? The heat capacity of steam is 2.01 J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).
What is the entropy change of the universe (in J K-1)when 2.00 mol of liquid water...

What is the entropy change of the universe (in J K-1)when 2.00 mol of liquid water at 0 °C freezes in a freezer compartment whose temperature is -15 °C? Assume the freezer is a perfect insulator. (AHfus = 6.01 kJ mol-1 for water) Select one: O a. +90.6 O b. +46.6 C. -2.6 O d. -44.0 o e. +2.6

Determine the change in entropy of the universe,in J/k when 2 moles of nitrogen at 20...

Determine the change in entropy of the universe,in J/k when 2 moles of nitrogen at 20 C are expanded isothermally in a piston-cylinder device with a change in pressure from 2 to 1 bar.The heat loss to the surroundings at 20 C is 3.4 kJ
References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is...

References Calculate the change in entropy that occurs when 18.02 g of ice at -12.5C is placed in 45,04 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 JK-mol-and 753 JK mol", respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy - JK Submit Answer T ry Another Version 3tem attempts remaining
Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed...

Calculate the change in entropy that occurs when 18.02 g of ice at –17.5°C is placed in 90.08 g of water at 100.0°C in a perfectly insulated vessel. Assume that the molar heat capacities for H2O(s) and H2O(l) are 37.5 J K^-1 mol^-1 and 75.3 J K^-1 mol^-1, respectively, and the molar enthalpy of fusion for ice is 6.01 kJ/mol. Change in entropy = ______J/K

What is the entropy change in the surroundings when one mole of ice melts at 0.00'C...

What is the entropy change in the surroundings when one mole of ice melts at 0.00'C in a large room maintained at 27.0°C? The heat of fusion of ice is 6.31 kJ/mol (answer in 1/K) Answer: 21.0 Check Finis
What is the entropy change to the surroundings when 1 mol of ice melts in someone's...

What is the entropy change to the surroundings when 1 mol of ice melts in someone's hand if the hand temperature is 32°C? Assume a final temperature for the water of 0°C. The heat of fusion of ice is 6.01 kJ/mol. a. -188 J/K b. -22.0 J/K c. -19.7 J/K d. +19.7 J/K e. +188 J/K
Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of...

Calculate the change in entropy (in J/K) that occurs when a sample containing 2.00 moles of water is heated from 10.00°C to 300.0 °C at 1 atm pressure. Molar Heat Capacity H2O(1) = 75.3 JK' moi? H2O(g) = 36.4 JK' mol Enthalpy of Vaporization at 100 °C = 40.7 kJ mol .-1 -1 Answer: