Final Temperature of Ice and Water Mixture - How Many Grams of Ice Will Melt? | Summary and Q&A

TL;DR

Learn how to calculate the final temperature of an ice-water mixture using specific heat capacities and enthalpy of fusion.

Key Insights

• 🥶 The final temperature of an ice-water mixture depends on whether some or all of the ice melts.
• 🫠 Calculations involve determining the energy required for heating, melting, and cooling/ heating in an ice-water mixture.
• 🥶 The energy absorbed by the ice and released by the water must be equal when the final temperature is reached.
• 🈂️ The enthalpy of fusion of ice (333 J/g) is used to calculate the energy required to melt the ice.
• 🥵 Specific heat capacity is used to calculate the energy required for heating or cooling the ice and water.
• 🤘 Adding a negative sign to the equation ensures the correct direction of energy transfer.

Transcript

in this video we're going to talk about how to determine the final temperature of an ice water mixture so in this example we have 25 grams of ice dropping into 50 grams of water so if you want a picture here's a visual so let's say this is the liquid water at 30 degrees celsius and then we have an ice cube dropped into it at negative 20. so because... Read More

Questions & Answers

Q: How does the final temperature of an ice-water mixture depend on whether some or all of the ice melts?

If only some of the ice melts, the final temperature will be 0 degrees Celsius. If all of the ice melts, the final temperature will be above 0 degrees Celsius.

Q: What equations are used to calculate the energy required for heating, melting, and cooling/ heating in an ice-water mixture?

In the case of partial melting, equations include q1 (energy to heat ice), q2 (energy to melt ice), and q3 (energy to cool water). In the case of complete melting, the equations include q1, q2, and q4 (energy to heat water).

Q: How can you determine if all of the ice will melt in an ice-water mixture?

Compare the energies absorbed by the ice (q1+q2) and released by the water (q4). If the energy absorbed is greater, all of the ice will melt; otherwise, only some will melt.

Q: How can you calculate how many grams of ice will melt in an ice-water mixture?

Divide the energy required to melt the ice (q2) by the enthalpy of fusion of ice (333 J/g). The result will be the mass of ice that melts.

Summary & Key Takeaways

• When ice is added to water at a higher temperature, heat flows from the water to the ice, causing the water temperature to decrease and the ice temperature to increase.

• The final temperature of the mixture depends on whether only some or all of the ice melts.

• Calculations involve determining the energy required to heat the ice, melt the ice, and cool/heat the water, depending on the situation.