The heat of combustion of glycogen is about 432 kJ/mol of carbon. Assume that average rate of heat l — Thermodynamics and Thermochemistry Chemistry Question
Question
The heat of combustion of glycogen is about 432 kJ/mol of carbon. Assume that average rate of heat loss by an adult male is 150 W. If we were to assume that all the heat comes from the oxidation of glycogen, how many units of glycogen (1 mole carbon per unit) must be oxidized per day to provide for this heat loss?
Answer: 0030
💡 Solution & Explanation
Heat loss rate = $150\text{ W} = 150\text{ J/s}$. Total energy required per day = $150 \times 24 \times 3600 = 12,960,000\text{ J} = 12960\text{ kJ}$. Heat provided per unit of glycogen = $432\text{ kJ}$. Number of units = $12960 / 432 = 30$. Format as 0030.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes