**Problem Statement:**How much would the temperature of 295 g of water increase if 17.4 kJ of heat were added? (The specific heat of liquid water is: 4.184 J/g °C)**Solution:**To calculate the temperature increase ($\Delta T$) when a certain amount of heat ($Q$) is added to a given mass ($m$) of water, we can use the specific heat capacity formula:\[ \Delta T = \frac{Q}{m \cdot c} \]Where:- $Q$ is the heat added (in joules)- $m$ is the mass of the water (in grams)- $c$ is the specific heat capacity of the substance (for water, $4.184 \, \text{J/g} \, ^\circ\text{C}$)Given values:- Mass of water ($m$): 295 g- Heat added ($Q$): 17.4 kJ = 17,400 J (since 1 kJ = 1000 J)- Specific heat capacity of water ($c$): 4.184 J/g °CBy substituting these values into the formula:\[ \Delta T = \frac{17,400\, \text{J}}{295\, \text{g} \times 4.184\, \text{J/g} \, ^\circ\text{C}} \]\[ \Delta T = \frac{17,400}{1233.28} \, ^\circ\text{C} \]\[ \Delta T \approx 14.1 \, ^\circ\text{C} \]So, the temperature of the 295 g of water would increase by approximately 14.1 °C if 17.4 kJ of heat were added.

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Answered: How much would the temperature of 295 g…

How much would the temperature of 295 g of water increase if 17.4 kJ of heat were added? (the specific heat of liquid water is: 4:184 J/g °C

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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