explains how the ice keeps a beverage cold. Thermodynamics Melting Energy Freezing
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Explain how ice cubes cool down beverages.
A large -20°C ice cube is dropped into a super-insulated container holding a small amount of 5°C water, then the container is sealed. Ten minutes later, the temperature of the ice (and any water that has melted from the ice) will be warmer than -20°C. This is a consequence of the second law of thermodynamics.
Adam M.
Thermodynamics Practice Problems: A 6-pack of 12 fl oz. soda cans is placed inside an insulated container. Ice is added to the container in order to chill the soda. What is the minimum amount of ice needed in order to cool the soda from room temperature (20°C) down to 4°C? Assume the container is a perfect insulator and ignore the presence of the cans themselves. Givens: Csoda = 4184 J/(kg·°C) Cice @ ~5°C = 2027 J/(kg·°C) Tinitial (ice) = -5°C List known values (convert if necessary): 1 fl oz. = 0.0295 L = 0.0295 kg List unknown values: Select equations: Substitute and solve:
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