**Heat Production and Temperature Regulation in Humans**An average human produces about 10 MJ of heat each day through metabolic activity. If a human body were an isolated system with a mass of 65 kg, having the heat capacity of water, what change in temperature would the body experience?Human bodies are actually open systems, and the main mechanism of heat loss is through evaporative cooling. What mass of water should be evaporated each day to maintain constant temperature?- \( C_{p,m} \) (water) = 75.29 J/K·mol- \( q_p = C_p \Delta T = nC_{p,m} \Delta T \)- \( \Delta H_{\text{evaporation}} = 44.016 \times 10^3 \) J/mol**Explanation:**- **Specific Heat Capacity (\( C_{p,m} \))**: This value is for water and indicates the amount of heat needed to raise the temperature of one mole of water by 1 Kelvin (K).- **Heat Quantification (\( q_p \))**: This equation calculates the heat gained or lost by the system, considering the specific heat capacity (\( C_p \)), change in temperature (\( \Delta T \)), and moles of substance (\( n \)).- **Heat of Evaporation (\( \Delta H_{\text{evaporation}} \))**: This is the amount of energy required to convert one mole of liquid water into vapor at constant temperature and pressure.The exercise challenges students to calculate how much water needs to be evaporated to counterbalance the heat produced through metabolism, ensuring that the body's temperature remains stable.

The objective of the question is to calculate the Temperature Mass of water

An average human produces about 10 MJ of heat each day through metabolic activity. IF a human body were an isolated system of mass 65 kg with the heat capacity of water, what temperature would the body experience? Human bodies are actually open systems, and the main mechanism of heat loss is through evaporative cooling. What mass of water should be evaporated each day to maintain constant temperature? Cp,m (water) = 75.29 J/K-mol qp = CpAT = nCp,mAT AHevaporation = 44.016 x 10³J/mol

An average human produces about 10 MJ of heat each day through metabolic activity. IF a human body were an isolated system of mass 65 kg with the heat capacity of water, what temperature would the body experience? Human bodies are actually open systems, and the main mechanism of heat loss is through evaporative cooling. What mass of water should be evaporated each day to maintain constant temperature? Cp,m (water) = 75.29 J/K-mol qp = CpAT = nCp,mAT AHevaporation = 44.016 x 10³J/mol

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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Exergonic Reaction

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Question

**Heat Production and Temperature Regulation in Humans**

An average human produces about 10 MJ of heat each day through metabolic activity. If a human body were an isolated system with a mass of 65 kg, having the heat capacity of water, what change in temperature would the body experience?

Human bodies are actually open systems, and the main mechanism of heat loss is through evaporative cooling. What mass of water should be evaporated each day to maintain constant temperature?

- \( C_{p,m} \) (water) = 75.29 J/K·mol
- \( q_p = C_p \Delta T = nC_{p,m} \Delta T \)
- \( \Delta H_{\text{evaporation}} = 44.016 \times 10^3 \) J/mol

**Explanation:**

- **Specific Heat Capacity (\( C_{p,m} \))**: This value is for water and indicates the amount of heat needed to raise the temperature of one mole of water by 1 Kelvin (K).
- **Heat Quantification (\( q_p \))**: This equation calculates the heat gained or lost by the system, considering the specific heat capacity (\( C_p \)), change in temperature (\( \Delta T \)), and moles of substance (\( n \)).
- **Heat of Evaporation (\( \Delta H_{\text{evaporation}} \))**: This is the amount of energy required to convert one mole of liquid water into vapor at constant temperature and pressure.

The exercise challenges students to calculate how much water needs to be evaporated to counterbalance the heat produced through metabolism, ensuring that the body's temperature remains stable.

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