### Experiment Data: Heating Cold and Hot Water#### Heating Cold Water:1. **Mass of Beaker and Cold Water**: 199.74 g2. **Mass of Beaker**: 107.36 g3. **Mass of Cold Water**: 92.38 g4. **Final Temperature of Cold Water**: 90°C5. **Initial Temperature of Cold Water**: 21°C6. **Change in Temperature**: 69°C7. **Elapsed Time**: 324 seconds#### Heating Hot Water:1. **Mass of Beaker and Hot Water**: 199.75 g2. **Mass of Beaker**: 107.36 g3. **Mass of Hot Water**: 92.39 g4. **Final Temperature of Hot Water**: 90°C5. **Initial Temperature of Hot Water**: 45°C6. **Change in Temperature**: 45°C7. **Elapsed Time**: 206 seconds### Summary:This data represents an experiment comparing the heating of cold and hot water. It details the masses involved, temperature changes, and the time taken to reach final temperatures. The cold water experienced a greater change in temperature over a longer period, while the hot water reached the same final temperature more quickly. **Question:**3. Calculate the amount of energy (in calories) needed to heat the hot water. Use the heat equation and specific heat of liquid water from Chapter 3. Show your work.**Solution Explanation:**The task is to calculate the energy required to heat water using the specific heat capacity. The equation used is typically:\[ Q = m \cdot c \cdot \Delta T \]- **Q** represents the heat energy (in calories).- **m** is the mass of the water (in grams).- **c** is the specific heat capacity of water (1 cal/g°C for liquid water).- **ΔT** is the change in temperature (final temperature - initial temperature, in °C).**Provided Calculation:**- The equation written appears to be: \[ Q = 45 \, \text{g} \times 1 \, \text{cal/g°C} \times 10 \,^\circ\text{C} \]The answer to this calculation, indicated in the image, is:- **Q = 450 calories**This represents the total energy needed to heat the given amount of water by the specified temperature change.

Given: Mass of hot water = 92.39 g. Change in temperature of hot water = -45 oC…

3. Calculate the amount of energy (in calories) needed to heat the hot water. Use the heat equation and specific heat of liquid water from Chapter 3. Show your work. ulov ert eleluols Jmlg ser0e.0 el 0 0.00 ts 1elew to ier phow Tuoy wode boleer

3. Calculate the amount of energy (in calories) needed to heat the hot water. Use the heat equation and specific heat of liquid water from Chapter 3. Show your work. ulov ert eleluols Jmlg ser0e.0 el 0 0.00 ts 1elew to ier phow Tuoy wode boleer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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