experiment 6: specific heat capacity Flashcards
It is the quantity of heat requires to raise the temperature of the body by 1 degree Celsius
Heat capacity of a body
- how much heat you need to raise the temperature of an entire object by a certain amount
It is defined as the heat per unit mass per degree change in temperature.
Specific heat of a substance
- tells you how much heat is needed to raise the temperature of just one unit of mass (like one kilogram) of a substance by one degree (1°C)
True or false:
the quantity of heat lost by the warmer body is equal to the heat gained by the cooler body, and some intermediate equilibrium temperature is finally reached.
In the second part of this lab, you will be measuring the latent heat of fusion of water. In this context,
“fusion” means “melting.” Phase changes, such as going from solid to liquid or liquid to gas, require energy.
True - When you have two objects at different temperatures (one hot and one cold) and you put them together, heat moves from the hot object to the cold one.
The heat that the hot object loses is exactly equal to the heat that the cold object gains. This continues until they reach the same temperature, called the equilibrium temperature.
Fusion means
Melting
What happens in the latent heat of fusion of water.
Phases changes like going from
S to L
L to G
they require energy
Formula of specific heat
c= Q/ m⋅Δt
c = specific heat (how much heat per unit mass per degree)
Q = total heat added
m = mass of the substance
∆t = change in temperature (how much the temperature increases)
What equipment is needed to measure the mass of the metal sample
Top-loading balance
Mcal
Calorimeter
(It’s like a metal cylinder tin)
Fill how much of water in the inner calorimeter
One-third of its volume
Fill how much of water in the inner calorimeter
One-third of its volume
Calculate Mw
to find the mass of water
Get the difference btwn Mcal+water and Mcal
Calculate Mw
How to find the mass of water
How do you measure the temperature
Using the temperature probes
Tw
Initial temperature of water
Tsample
Temperature of metal sample
What should you do after measuring the temperature of the metal sample
Remove the metal sample from the boiling water
Quickly wipe it dry
Suspend it in water in the calorimeter
Sample should be immersed in water but not touching the bottom of the calorimeter
Find change in Tw
∆𝑻𝒘 = 𝑻𝒇 − 𝑻𝒘
Find the change in temperature of metal sample
∆𝑻𝒔𝒂𝒎𝒑𝒍𝒆 = 𝑻𝒔𝒂𝒎𝒑𝒍𝒆 − 𝑻𝒇
Determine the specific heat of metal sample by applying the law of heat exchange
Heat gained by water = Heat lost by metal sample
𝑸𝒈𝒂𝒊𝒏𝒆𝒅 = 𝑸𝒍𝒐𝒔𝒕
Determine the specific heat of metal sample by applying the law of heat exchange
Heat gained by water = Heat lost by metal sample
𝑸𝒈𝒂𝒊𝒏𝒆𝒅 = 𝑸𝒍𝒐𝒔𝒕
What is the specific heat of the metal sample
𝒄𝒔𝒂𝒎𝒑𝒍𝒆 = M𝒘C𝒘∆𝑻𝒘 +M𝒄𝒂𝒍C𝒄𝒂𝒍∆𝑻𝒄𝒂𝒍
/M𝒔𝒂𝒎𝒑𝒍𝒆 ∆𝑻𝒔𝒂𝒎𝒑𝒍𝒆
How many grams of ice
Btwn 10 and 30 grams
Or
Size of a teaspoonful
Or
Couple of grapes
- If the sample of ice is too large, the ice will not melt completely and you will have
to repeat the experiment with a smaller sample.
True or false:
The ice should be at 0°C when you put it in the calorimeter.
True - If the ice was taken fresh from a freezer, it might be colder. If that is the case, let the ice rest on the table until it starts to melt
What happens if there is water on the ice
Remove the excess water from the ice and just before putting the ice into the calorimeter
What equipment is used to weigh the thermal equilibrium
GLX
Compute the latent heat of fusion of water.
Heat Gained = Heat Lost
(Heat that enters the ice) + (Heat that enters the ice water) = (Heat lost by the cup) + (Heat lost by the stirrer) + (Heat lost by the cup water)
Where do we place the
Warm water -
Ice water -
Warm water - into the calorimeter cup
Ice water - it is the source of thermal energy
What is the general eqn for latent heat
Q=mL
m is the mass of the substance
L is the latent heat
