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Understanding Heat Transfer: Basics of ΔT, q, and Energy Conversion

This overview of heat transfer quantifies temperature changes using the equation ΔT = Tfinal – Tinitial and relates heat energy to mass and heat capacity. We explore key concepts such as heat energy measured in joules, specific heat capacity in joules/gram•°C, and the distinction between endothermic and exothermic processes. By understanding how to calculate heat (q = mCΔT) and converting energy units from calories to joules, you will grasp the essential principles behind thermal energy and its real-world applications.

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Understanding Heat Transfer: Basics of ΔT, q, and Energy Conversion

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  1. Quantifying Heat The Math!

  2. Equation change in temperature, measured in °C ΔT = Tfinal – Tinitial heat energy – measured in joules (J) heat capacity – how much heat a substance can hold, measured in joules/gramdegrees Celsius mass - measured in grams (g) q = mCΔT

  3. Units for heat (q) Most food tells us the amount of energy in units of Calories. . . . Calories are kilocalories (1 Cal = 1000cal) The SI unit for energy is Joules (J) 1 cal = 4.184 J Let’s do some quick conversions.

  4. How can you tell if a process is endothermic or exothermic? Endothermic Exothermic q is a negative number Why? The final temperature is lower than the initial temperature- heat was given off from the system. ΔT = Tfinal – Tinitial • q is a positive number • Why? • The final temperature is higher than the initial temperature- we added heat to the system. • ΔT = Tfinal – Tinitial Let’s solve some problems!

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