Specific Heat
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Specific heat represents the amount of heat required to change a unit mass of a substance by one degree Celsius. This is expressed mathematically as:
#q = m * c * DeltaT# , where#q#  the amount of heat supplied;
#m#  the mass of the substance;
#c#  the respective substance's specific heat;
#DeltaT#  the change in temperature.So, if we want to determine the units for specific heat, we'll just isolate the term in the above formula to get
#c = q/(m * DeltaT)# . Since heat is measured in Joules (J), mass in grams (g), and temperature in degree Celsius (#C# ), we can determine that#c = J/(g * ^@C)# .Therefore, specific heat is measured in Joules per g times degree Celsius.

Specific heat is an intensive property (like density, color, etc.) that does not depend on the amount of a substance present. This allows substances to be identified using their specific heat.
Imagine an unknown metal of known mass is heated to a known temperature. The heated metal can then be placed into a sample of water for which the volume (and therefore mass since 1mL=1g) and temperature are known.
The amount of energy (Q) transferred to the water can be calculated by using the equation
#Q_w=m_wCâˆ†T_w# since the mass (m) and âˆ†T(temp change) can be measured.This allows for a calculation of the C value for the metal since the head gained (Qw) of the water will equal the heat lost by the metal (Qm).
The C value for the metal allows the metal to be identified.
A listing of C values for metals can be found here:
http://www2.ucdsb.on.ca/tiss/stretton/database/Specific_Heat_Capacity_Table.html
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Thermochemistry

1Energy Change in Reactions

2Enthalpy

3Exothermic processes

4Specific Heat

5Calorimetry

6Thermochemistry of Phase Changes

7Thermochemistry with Equation Stoichiometry

8Hess' Law

9Spontaneous and NonSpontaneous Processes

10Entropy

11Gibbs Free Energy

12Endothermic processes

13BornHaber Cycle  Formation

14BornHaber Cycle  Solution