Energy Changes in Chemical Reactions (HSC SSCE Chemistry): Flashcards
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State when thermal equilibrium is reached
State when thermal equilibrium is reached
When two objects in contact reach the same temperature
Relation between °C and K for temperature changes
Relation between °C and K for temperature changes
A change of 1°C equals a change of 1 K
Difference between temperature and quantity of heat
Difference between temperature and quantity of heat
Temp. is how hot; quantity of heat is total thermal energy
First principle: heat energy relation to mass
First principle: heat energy relation to mass
Amount of heat energy is proportional to the mass
Second principle: heat in equal masses of different substances
Second principle: heat in equal masses of different substances
Depends on the nature of the substances involved
Define specific heat capacity ()
Define specific heat capacity ()
Heat to raise unit mass by 1°C (or 1 K)
Specific heat capacity of water in
Specific heat capacity of water in
4.18 (highest of common substances)
Equation to calculate quantity of heat
Equation to calculate quantity of heat
What does positive indicate?
What does positive indicate?
Heat gained (endothermic, temperature increased)
What does negative indicate?
What does negative indicate?
Heat lost (exothermic, temperature decreased)