The conversion of solid CO2 ("dry ice") to CO2 gas is product-favored at room temperature. What would be the signs for ΔG, ΔH, and ΔS at room temperature?
CO2(s) --> CO2(g)
ΔG = (+) ΔH = (+) ΔS = (-)
ΔG = (-) ΔH = (+) ΔS = (-)
ΔG = (+) ΔH = (+) ΔS = (+)
ΔG = (-) ΔH = (+) ΔS = (+)
ΔG = (-) ΔH = (-) ΔS = (+)
The conversion of solid CO2 ("dry ice") to CO2 gas is product-favored at room temperature. What...
The dissolving of CaCl2 in water is product-favored, but the temperature of the water gets colder during the process. What would be the signs for ΔG, ΔH and ΔS during this process? CaCl2(s) ---> Ca+2(aq) + 2Cl-1(aq) ΔG = (+) ΔH = (+) ΔS = (-) ΔG = (-) ΔH = (-) ΔS = (+) ΔG = (-) ΔH = (+) ΔS = (-) ΔG = (-) ΔH = (+) ΔS = (+) ΔG = (+) ΔH = (+) ΔS = (+)
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?
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.
30 g of dry ice (solid CO2) is placed in a 2.0×104 cm3 container, then all the air is quickly pumped out and the container sealed. The container is warmed to 0∘C, a temperature at which CO2 is a gas. a.) What is the gas pressure? Give your answer in atm. The gas then undergoes an isothermal compression until the pressure is 2.4 atm , immediately followed by an isobaric compression until the volume is 2000 cm3 . b.) What...
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.
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.
1 Review l Constants Part A 30.0 g of dry ice (solid CO2) is placed in a container which has an initial volume 2.00x104 cm. then all the air is quickly pumped out and the container is sealed. The container is warmed to 0°C-a ternperature at which CO2 is a gas. How many moles of CO, were placed in the container? EVO AXO th 0 ? 12 = moles Submit Request Answer Part B What is the gas pressure? Give...
13) (1.5 pts) You fill an uninflated balloon with 18 grams of solid CO2 (dry ice, M= 44.0 g/mol). What volume will the dry ice occupy when it vaporizes at 25°C and 1.02 atm? The balloon has capacity of 6.5 liters, will it pop?
3. A 1.20-g sample of dry ice is added to a 755 ml flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas), and the mixture returns to 25.0 °C. What is the total pressure in the flask? MISSED THIS? Read Section 6.6; Watch KCV 6.6
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.)