• Determining The Heat of Fusion For Ice
• https://youtu.be/agCwGODs8ms 
• The Heat of Fusion ( Q_f ), is the amount of heat energy required to melt a gram of ordinary ice. In this demonstration, we will be determining this by placing a known mass of ice at 0 degrees Celsius, into a known initial mass of water at a known temperature. We will then measure the change or drop, in temperature in order to determine the heat of fusion.
• First, we must again assume that the Heat gained is equal to the heat that is lost. Heat is lost by the water, to not only melt the ice, but to take that volume of zero degree ice water, and raise it up to the final temperature.  
• We then have:
• Q lost by the water = Q gained by the ice in melting   +  Q gained by the 0 degree water from the melted ice to reach the final temperature (T_f )
• We then have:
• c of water m of the initial water ∆T of the initial water to the final temperature ₌ 
• Q_f mof the ice  +    c of water m of ice water from the melted ice  ∆ T of the melted ice water (presumed to be at 0 degrees Celsius), to the final temperature.
• In the demonstration, we will proved all of the information needed, in order to determine the value of Q_{f .}
• _{Things To Do}
• 1. You are to use these values in order to calculate the Heat of Fusion for Ice. Explain how you got your answer.
• 2. Look up the actual Heat of Fusion for Ice (or note from video).
•    What is the percent difference ?  In other words, how far were you off in terms of percent, from the actual value? [Show calculation]
• 3. What do you think caused the greatest amount of this error?
•  

Determining The Specific Heat of a Substance

•  Determining The Specific Heat of a Substance 
• https://youtu.be/XdbaeZO2WGU 
• The Specific Heat of a substance is defined as the amount of energy (usually expressed in calories), that it takes to change the temperature of a gram of that substance, one degree Celsius.  In the case of water, it takes 1 calorie of energy to elevate or lower a gram of water, one degree, Celsius, so the Specific Heat ( c ) is 1.  This is given by the formula:
• Q = c m  ∆ T 
• Where Q is the total heat, c is the specific heat, m is the mass of the substance in grams, and   ∆ T is the temperature change the substance goes through. 
• In this demonstration, we will place some hot Copper into some room temperature water. The water will heat up, and at the same time, the Copper will cool down to a final temperature. We will use the Conservation of Energy theorem to understand that the energy gained by the water, will be the same as the energy lost by the hot Copper.
• Q gained by the water = Q lost by the hot Copper 
• Therefore: 
• c water m water  ∆ T water   =   c Copper m Copper ∆ T Coppe
• In the demonstration, we will use two stacked foam cups, which will be our calorimeter. For the purpose of this demonstration, we shall treat the calorimeter as not being involved in reaching a final temperature. In reality, there is no such thing as a 100% insulated vessel, and so the calorimeter would either gain or lose a small amount of heat energy, and would need to be factored into our calculations.  
• The change in temperature of the water will be the final temperature of the water minus the initial temperature of the mixture, because the water will gain energy. The change in temperature of the Copper will be the initial temperature of the Copper minus the final temperature of the mixture, because the Copper will be losing energy. The initial temperature of the Copper, is 100 degrees Celsius because it is being heated to the boiling point of water (100 degrees Celsius), before it is immersed into the room temperature water.
• In the demonstration, you will be given all of the values you need to find everything except the specific heat of the Copper.
•  
• Things To Do
• 1. You are to use these values in order to calculate the Specific Heat of Copper. Explain how you got your answer..
• 2. Look up the actual Specific Heat of Copper.
•    What is the percent difference ?  In other words, how far were you off in terms of percent, from the actual value? [Show calculation]
• 3. What do you think caused the greatest amount of this error?

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Status NEW Posted 17 Jun 2017 12:06 AM My Price 12.00

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