Dry Ice. At standard atmospheric pressure, the solid form of carbon dioxide called “dry ice” undergoes a phase change not to a liquid but straight to a gas. This process is called sublimation, and like other phase transitions heat energy is required. In this case it is the latent heat of sublimation, which for carbon dioxide is 573 kJ/kg at the sublimation temperature of 78.5 °C. If 118 g of dry ice is dropped into 0.51 liters water at room temperature (20 °C), how much of the water will turn to ice by the time all the dry ice has sublimated? Note that when the dry ice becomes a gas, the gas bubbles out of the system.

Question

Dry Ice. At standard atmospheric pressure, the solid form of carbon dioxide called “dry ice” undergoes a phase change not to a liquid but straight to a gas. This process is called sublimation, and like other phase transitions heat energy is required. In this case it is the latent heat of sublimation, which for carbon dioxide is 573 kJ/kg at the sublimation temperature of ­78.5 °C. If 118 g of dry ice is dropped into 0.51 liters water at room temperature (20 °C), how much of the water will turn to ice by the time all the dry ice has sublimated? Note that when the dry ice becomes a gas, the gas bubbles out of the system.