Final answer:
The question pertains to the thermal energy transfer between an ice cube and water leading to an equilibrium temperature. The pertinent calculations involve the mass of the ice and water, their specific heat capacities, and the heat of fusion of ice.
Step-by-step explanation:
The student's question involves understanding the transfer of thermal energy or heat between an ice cube at 0 °C and a quantity of water at 21 °C, leading to the melting of the ice cube and the subsequent equilibrium temperature of the combined water system. To solve this problem, we can use the principles of conservation of energy and the concept of specific heat and heat of fusion. The amount of heat required to melt the ice cube (heat of fusion) must be equal to the heat lost by the warmer water as it cools down, and no heat is exchanged with the environment.
The temperature of the water after the ice has melted will depend on the specific heat capacities of the ice and water, the mass of the ice and water, and the heat of the fusion of ice. To reiterate, the question asked was: 'You place an ice cube with a mass of 82 g into a glass with 881 g of water. The ice cube was at 0 °C, and the water was at 21 °C. After the ice has melted, what would be the temperature of the water in the glass?' The correct option corresponding to that situation will be the resulting equilibrium temperature after calculations based on the aforementioned thermodynamic properties.