If a calorimeter has a mass of 6.0 g, a specific heat of 2.0 J/(g*C), and it and its contents undergo a temperature increase of 5.5 *C, how much heat is gained by the calorimeter?
q = heat gained = mass x specific heat x delta T.
To determine the heat gained by the calorimeter, we can use the formula:
Q = m * c * ΔT
where:
Q is the heat gained (or lost),
m is the mass of the calorimeter and its contents,
c is the specific heat of the calorimeter and its contents, and
ΔT is the change in temperature.
In this case, the mass of the calorimeter is given as 6.0 g, the specific heat is 2.0 J/(g*C), and the change in temperature is 5.5 *C.
Now we can substitute the given values into the formula to calculate the heat gained by the calorimeter:
Q = 6.0 g * 2.0 J/(g*C) * 5.5 *C
First, we multiply the value for mass (6.0 g) by the value for specific heat (2.0 J/(g*C)), which gives us 12.0 J/C. Then, we multiply this result by the change in temperature (5.5 *C), resulting in:
Q = 12.0 J/C * 5.5 *C
To simplify the calculation, we can cancel out the units of degrees Celsius, which gives us:
Q = 12.0 J * 5.5
Now we multiply 12.0 J by 5.5, resulting in:
Q = 66 J
Therefore, the calorimeter gained 66 Joules (J) of heat.