The question is incomplete, the complete question is;
In the Energy and Specific Heat lab, you measure the temperature change of water to study the specific heat of a metal. What statement explains the relationship between the water and the metal you are studying? Select one: O The heat lost by the metal plus the heat gained by the water equals 100. O The temperature change of the metal is equal to the temperature change of the water. O The heat lost by the metal is equal to the heat gained by the water. The initial temperature of the metal equals the initial temperature of the water
Answer:
The heat lost by the metal is equal to the heat gained by the water.
Explanation:
When the piece of metal is put into water, heat is lost by the metal and gained by the water.
Recall that energy is conserved hence heat lost by metal must be equal to heat gained by water.
Thus, the relationship between the metal under study and the water is that the metal looses heat to the water and heat lost by metal is equal to heat gained by water.
A “supersaturated” solution contains more dissolved material. supersaturated solutions lies in the temperature of the water. more sugar will dissolve in hot water than in cold. Meaning that by separating the 2, only the supersaturated sugar would dissolve leaving the regular sugar untouched.
Answer:
the number of possible configurations of the locations and energies of the atoms or molecules that comprise a system
Explanation:
Ludwig Boltzmann was the first to suggest that the concept of entropy could be calculated by examining the positions and energies of molecules. This was developed into an equation, known as the Boltzmann equation, which relates entropy to the number of microstates (W):
S = k ln W
where k is the Boltzmann constant (1.38 x 10-23 J/K), and W is the number of microstates.
Microstates was used to imply the number of different possible arrangements of molecular position and kinetic energy at a particular thermodynamic state. Therefore any process that gives an increase in the number of microstates therefore increases the entropy. Hence the answer.
From the gas law, PV=nRT we can say that P(pressure), V(volume) and T (temperature) are related to each other. The initial volume of sample is 408 ml
Given that initial volume of the sample = V1
initial pressure of the sample = 0.92atm
initial temperature of the sample = 23.2oC
Final pressure of the sample = 1.3atm
Final temperature of the sample = 40.1 oC
Final volume of the sample = 500ml = 0.5L
Using the relation P1V1/T1 = P2V2/T2
V1 = 1.3x0.5x23.2/40.1x0.92 = 15.08/36.892 = 0.408
Hence the initial volume of sample = 408 ml
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