Specific Heat Capacity

Core Concept

Specific Heat Capacity (c) is the amount of heat required to raise the temperature of 1 gram of a substance by 1°C. This property varies between substances and is crucial in understanding how different materials absorb and transfer heat.

  • Keep Units Consistent: Ensure mass is in grams, temperature in Celsius, and heat in Joules unless specified otherwise.

  • Pay Attention to ΔT: Always use the correct difference between final and initial temperatures, especially when finding temperature changes.

  • High vs. Low Specific Heat: Remember, substances with high specific heat capacity require more energy to change temperature and vice versa.

  • Account for the Substance’s Phase: The specific heat capacity can vary significantly between solid, liquid, and gas phases of the same substance.

Test Yourself

Assorted Multiple Choice
A constant current is passed through an electrolytic cell for 45.0 minutes, delivering a total charge of 8,100 Coulombs. How many moles of electrons were transferred during this process? (Faraday's constant = 96,485 C/mol e⁻)

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Specific Heat Capacity

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Key Concepts of Specific Heat Capacity

Definition:

  • Specific heat capacity (c) measures the thermal energy a substance can absorb per unit of mass for each degree of temperature increase.

  • It is typically measured in Joules per gram per degree Celsius (J/g °C) or calories per gram per degree Celsius (cal/g °C).

Formula for Heat Transfer:

  • The formula to calculate the amount of heat (qqq) absorbed or released by a substance is: q = m⋅c⋅ΔT

  • Where:

    • q: Heat absorbed or released (in Joules or calories)

    • m: Mass of the substance (in grams)

    • c: Specific heat capacity of the substance

    • ΔT: Temperature change ($T_{\text{final}} - T_{\text{initial}}$)

Units:

  • J/g °C (Joules per gram per degree Celsius): Common unit in scientific contexts.

  • cal/g °C (calories per gram per degree Celsius): Often used in older scientific literature or in specific fields.

Understanding High vs. Low Specific Heat Capacity:

  • High Specific Heat Capacity: Substances with high specific heat can absorb a large amount of heat without a significant change in temperature. Example: Water (4.18 J/g °C).

  • Low Specific Heat Capacity: Substances with low specific heat capacity heat up or cool down quickly with small amounts of heat. Example: Metals like copper (0.385 J/g °C).

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