A chemist wants to calculate the amount of heat that is absorbed by a sample of copper as it is melted. Which constant should sh
1 answer:
The constant used for the absorption of heat by the sample in melting is . Thus, option A is correct.
The chemical reaction has been defined as the energy in which the energy has been released or absorbed for the breaking of bonds in the reactants and the formation of product.
<h3>Constant for energy absorbed</h3>The energy has been absorbed in the melting of the copper sample. Thus, the sample has been converted from the solid to the liquid state.
The change in energy with the conversion in solid and liquid state has been termed as heat of fusion.
The energy has been absorbed by the system, thus it has been marked with the positive sign.
Therefore, has been the constant used for the absorption of heat by the sample in melting. Thus, option A is correct.
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The mass of Copper deposited at the cathode : 0.296 g
<h3>Further explanation</h3>Given
time = t = 10 min=600 s
current = i = 1.5 A
F = 96500 C
charge Cu=+2
Required
The mass of Copper
Solution
Faraday's Law
e = Ar/valence(valence Cu=2, Ar=63.5 g/mol)
Input the value :
Data:
Q = 402.7 J → releases → Q = - 402.7 J
m = 16.25 g
T initial = 54 ºC
adopting: c = 4.184J/g/°C
ΔT (T final - T initial) = ?
Solving:
Q = m*c*ΔT
-402.7 = 16.25*4.184*ΔT
-402.7 = 67.99*ΔT
If: ΔT (T final - T initial) = ?
Q = 402.7 J → releases → Q = - 402.7 J
m = 16.25 g
T initial = 54 ºC
adopting: c = 4.184J/g/°C
ΔT (T final - T initial) = ?
Solving:
Q = m*c*ΔT
-402.7 = 16.25*4.184*ΔT
-402.7 = 67.99*ΔT
If: ΔT (T final - T initial) = ?