Suppose you place an ice cube in a cup of room-temperature water and then seal t

Question

Suppose you place an ice cube in a cup of room-temperature water and then seal them in a well-insulated container. No energy can enter or leave the container. If you open the container an hour later, which do you expect to find: a cup of water, slightly cooler than room temperature, or a large ice cube and some 100 degree C steam? Finding a large ice cube and some 100 degree C steam would not violate the first law of thermodynamics. W = 0 J and Q J, because the container is sealed, and delta E_th = 0 J because the increase in thermal energy of the water molecules that have become steam is offset by the decrease in water molecules that have turned to ice. Energy is conserved, yet we never see a process like this. Why not?

Explanation / Answer

a. cup of water slightly cooler than room temperature. because ice will receive heat and water will reject heat. so obviously, the resultant mixure will be hotter than ice but cooler than room temperature.

b. because although energy is conserved but it violates 2nd law of thermodynamics. Heat flows form higher temperature to lower temperature. In this case it travels in opposite direction. this violates 2nd law.

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