## Chapter 10 Section 10-5

 calorie
 the amount of energy (heat) required to raise thetemperature of one gram of water by one Celsius degree.1000 cal = 1 Caljoule: the SI unit.1 cal = 4.184 J
 Specific Heat Capacity
 The amount of energy required to changethe temperature of one gram of a substance by one Celsius degree.· Known as Specific Heat· Symbol Cp or s· Units: J/(goC) or cal/(goC)· Depends on Substance and State of Matter.· Some Common Cp’sWater (l) : 4.184 J/(goC)Water (s): 2.03 J/(goC)Aluminum: 0.89 J/(goC)Gold: 0.13 J/(goC)· Lower Cp responds faster to heating or cooling.
 Specific Heat Capacity Equation
 Q = s x m x (Tf – Ti)Q: Heats: Specific Heat Capacitym: MassTf: Final TemperatureTi: Initial TemperatureTf – Ti = Change in Temperature (Delta T)
 Heat problems involving more than one substance.
 The magnitude of the heat (Q) lost by one object is equal to themagnitude of the heat (Q) gained by the other object.· One object is exothermic the other is endothermic so the Q forone is positive while the Q for the other is negative.· Since they are the same magnitude but different signs, we can say0 = Q1 + Q2· In fact when multiple objects all at different temperatures aremixed in a sealed system, the objects transfer heat to each otheruntil they all reach the same final temperature. We assume noheat is lost or gained by the surroundings.0 = Q1 + Q2 + Q3 + … Qz
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