Answer:
As the specific heat capacity for pure diamond is 0.5091[tex]\frac{J}{g.K}[/tex] and it is different from the specific heat capacity found that is 0.2699[tex]\frac{J}{g.K}[/tex], the diamond sample is not pure.
Explanation:
1. As the problem says the equation that describes the amount of heat gained or lost by a substance is:
[tex]q=Cp*m*(T_{2}-T_{1})[/tex]
q=Cp*m*ΔT
where q is the amount of heat, Cp is the specific heat capacity, m is the mass and ΔT is the change in the temperature.
2. Solving for specific heat capacity:
[tex]Cp=\frac{q}{m*(T_{2}-T_{1})}[/tex]
3. Replacing values:
[tex]Cp=\frac{26.21J}{2.03g*(73.81C-25.99C}[/tex]
[tex]Cp=0.2699\frac{J}{g.K}[/tex]
As the specific heat capacity for pure diamond is 0.5091[tex]\frac{J}{g.K}[/tex] and it is different from the specific heat capacity found that is 0.2699[tex]\frac{J}{g.K}[/tex], the diamond sample is not pure.
The diamond sample is not pure because the specific heat capacity of pure diamond is 0.5091, it differs from the 0.2699 seen in other materials.
The heat capacity of a substance is the heat capacity of the substance divided by the mass of the substance.
Q = mcΔT
Q = heat energy
m = mass
c = heat capacity
T = change in temperature
In the equation, there is loss or gain of heat
[tex]c = \dfrac{Q}{m(T_2-T_1)}[/tex]
Putting the values
[tex]\rm c = \dfrac{26.21 J}{m(73.81^\circ C-25.99^\circ C)} = 0.2699 J/g.K[/tex]
Thus, the heat capacity is 0.2699 J/g.k
Learn more about heat capacity
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