Calculate the amount of heat required to completely sublime 58.0 g of solid dry ice (CO2) at its sublimation temperature. The heat of sublimation for carbon dioxide is 32.3 kJmol−1.
Calculate the amount of heat required to completely sublime 58.0 g of solid dry ice (CO2)...
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).
Your instructor gives you a 100 g of dry ice (solid carbon dioxide) at -100 °C. Through the course of an experiment, you end up with 100 g of gaseous carbon dioxide at 0 °C. Answer the following questions based on this data. Assume that no heat is lost to the outside environment during the experiment. The specific heats for solid and gaseous carbon dioxide are 0.296 and 0.203 cal/g-°C respectively. Remember, carbon dioxide sublimes from solid to gas at...
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.
The standard enthalpy of sublimation of dry ice (solid carbon dioxide) is 6.03 kJ/mol. The triple point of CO2 is at 5.1 atm, -56.7 °C. Calculate ΔSsublimation and ΔGsublimation at the triple point.
Please Help!!!! 13. Carbon dioxide (typically called dry ice when it?s in solid form) transitions between its solid phase and its gas phase at a temperature of -78.5 degree C. Suppose we have 3.12 kg of dry ice at -125 degree C. flow much heat must be added to transform all of the dry ice into gas with an equilibrium temperature of -78.5 degree C? The latent heat of sublimation of dry ice is 5.72 x 10^5 J/kg and the...
If 2.50 kg of dry ice (solid carbon dioxide) is added to 1 5.0 L of water with an initial temperature of 24.0 degree C what is the temperature of the water when all of the dry ice has sublimed? For CO_2, the enthalpy of sublimation is 25.2 kJ/mol.
1. A 4.40-g piece of solid CO, (dry ice) is allowed to sublime in a balloon. The final volume of the balloon is 1.00 L at 300 K. What is the pressure of the gas? A) 2.46 atm B) 246 atm C) 0.122 atm D) 122 atm E) none of these
Dry ice, CO2(s), is thermodynamically stable at temperatures below -78 °C. The sublimation of dry ice can be described by the following equation: CO2(s) = CO2(g) What are the signs for the enthalpy, entropy, and free energy change for the sublimation at room temperature? Justify your answer for each thermodynamic value.
A 41.1 g sample of solid CO2 (dry ice) is added to a container at a temperature of 100 K with a volume of 3.4 L. A. If the container is evacuated (all of the gas removed), sealed, and then allowed to warm to room temperature T = 298 K so that all of the solid CO2 is converted to a gas, what is the pressure inside the container?
What is the entropy change in J/K to the universe when a dry ice (CO2) sculpture weighing 386.1 g sublimates on a table top at 21.7 °C and the process occurs reversibly? The temperatures of the dry ice solid and vapour are both -78.5 °C, and the heat of sublimation of dry ice is 21.6 kJ/mol. (2 marks) (Give answer to 3 significant figures.)