a block of aluminum is placed in 10.0g of water. the initial temperature of the water is 22.0 degrees celcious and its final temperature is 27.0 degrees celcious. what is the amount of heat released by the block of aluminum in calories if it had an initial temperature of 48.0 degrees celsius? aluminum has a specific heat of .897J/degrees celsius
Note the correct spelling of celsius.
q = mass Al x specific heat Al x (Tfinal-Tinitial)
To calculate the amount of heat released by the block of aluminum, we can use the equation:
Q = mcΔT
Where:
Q is the amount of heat released or absorbed
m is the mass of the substance
c is the specific heat capacity of the substance
ΔT is the change in temperature
In this case, we want to find the amount of heat released by the block of aluminum. The mass of the block is not provided, so let's assume it is 1 gram for the purpose of this explanation.
First, let's calculate the change in temperature (ΔT) of the aluminum block. The initial temperature (Ti) of the block is given as 48.0 degrees Celsius, and the final temperature (Tf) of the water is given as 27.0 degrees Celsius:
ΔT = Tf - Ti
ΔT = 27.0°C - 48.0°C
ΔT = -21.0°C
Since the temperature change is negative, it means that the block of aluminum is losing heat to the water.
Next, let's plug in the values into the equation and calculate the amount of heat released by the block of aluminum:
Q = mcΔT
Q = (1g) × (0.897 J/g°C) × (-21.0°C)
Q = -18.837 J
However, we need to convert the heat value from joules to calories:
1 calorie = 4.184 joules
So, let's convert joules to calories:
Q = -18.837 J × (1 cal / 4.184 J)
Q ≈ -4.50 cal
Since the block of aluminum is releasing heat, the negative sign indicates the heat loss. Therefore, the amount of heat released by the block of aluminum is approximately 4.50 calories.