Answer:
a. Energy Absorbed by Water
The energy absorbed by the water can be calculated using the following equation:
Q = mcΔt
where:
* Q is the energy change in joules
* m is the mass of the water in grams
* c is the specific heat of water in J/g°C
* Δt is the change in temperature in °C
In this case, we have:
* m = 200.0 g
* c = 4.18 J/g°C
* Δt = 28.3°C - 25.3°C = 3.0°C
Plugging these values into the equation, we get:
Q = (200.0 g) * (4.18 J/g°C) * (3.0°C) = 2508 J
Therefore, the water absorbed 2508 J of energy from the metal.
b. Energy Change of Metal
The energy change of the metal can be calculated using the following equation:
Q = mcΔt
where:
* Q is the energy change in joules
* m is the mass of the metal in grams
* c is the specific heat of the metal in J/g°C
* Δt is the change in temperature in °C
In this case, we have:
* m = 43.8 g
* Δt = 100°C - 28.3°C = 71.7°C
We can rearrange the equation to solve for c:
c = Q / (mΔt)
Plugging in the values we know, we get:
c = 2508 J / (43.8 g * 71.7°C) = 0.83 J/g°C
Therefore, the energy change of the metal was -2508 J. The negative sign indicates that the metal lost energy as its temperature decreased.
c. Specific Heat of Metal
The specific heat of the metal is 0.83 J/g°C.
d. Identity of Metal
The specific heat of the metal is closest to that of aluminum, which is 0.90 J/g°C. Therefore, the metal is likely aluminum.
