Response:
The specific heat of the alloy
Clarification:
Weight of the alloy = 25 gm
Initial temperature = 100°c = 373 K
Weight of the water = 90 gm
Initial temperature of water = 25.32 °c = 298.32 K
Final temperature = 27.18 °c = 300.18 K
Using the energy balance equation,
Heat released by the alloy = Heat absorbed by the water
[[
-
] =
(
-
)
25 × × ( 373 - 300.18 ) = 90 × 4.2 (300.18 - 298.32)
This gives us the specific heat of the alloy.
Answer: The enthalpy change for the reaction is, 201.9 kJ
Explanation:
Based on Hess’s law of constant heat summation, the energy released or absorbed in a chemical reaction stays constant, regardless of whether the process unfolds in one step or multiple steps.
This principle implies, that chemical equations can be treated analogously to algebraic expressions, allowing addition or subtraction to create the needed equation. Thus, the overall enthalpy change corresponds to the summation of the individual enthalpy changes of the reactions occurring in between.
The balanced equation for appears as follows,
The intermediate balanced reactions are outlined as follows,
(1)
(2)
(3)
(4)
Next, we will multiply the first reaction by 2, reverse the second, and reverse and halve the third and fourth reactions before combining them. This gives us:
(1)
(2)
(3)
(4)
Therefore, the expression for the enthalpy of the reaction is,
Hence, the enthalpy change for this reaction is, 201.9 kJ