If 57j of heat are added to an aluminum can with a mass of 17.1g, what is its temperature change?
To calculate the temperature change of the aluminum can, we need to use the specific heat capacity formula:
q = m * c * ΔT
Where:
q = amount of heat transferred
m = mass of the object
c = specific heat capacity
ΔT = change in temperature
In this case, the specific heat capacity of aluminum is 0.897 J/g°C.
Let's plug in the values:
57 J = 17.1 g * 0.897 J/g°C * ΔT
Now, we can solve for ΔT:
ΔT = 57 J / (17.1 g * 0.897 J/g°C)
ΔT = 3.19 °C
Therefore, the temperature change of the aluminum can is 3.19 °C.
To find the temperature change of the aluminum can, we need to use the specific heat capacity of aluminum.
The specific heat capacity is the amount of heat energy required to raise the temperature of a substance by one degree Celsius (or one Kelvin).
For aluminum, the specific heat capacity is 0.897 J/g°C.
To find the temperature change, we can use the formula:
q = m * c * ΔT
Where:
q is the heat energy (in joules)
m is the mass of the substance (in grams)
c is the specific heat capacity (in J/g°C)
ΔT is the temperature change (in °C)
In this case, we know the heat energy (q) is 57 J and the mass (m) is 17.1 g.
Now, let's rearrange the formula to solve for ΔT:
ΔT = q / (m * c)
Plugging in the given values, we get:
ΔT = 57 J / (17.1 g * 0.897 J/g°C)
Calculating it, we have:
ΔT = 57 J / 15.3507 J/°C
ΔT ≈ 3.7159 °C
Therefore, the temperature change of the aluminum can is approximately 3.7159 degrees Celsius.