When using a calorimeter, the initial temperature of a metal is 70.4C. The initial temperature of the water is 23.6C. At the end of the experiment, the final equilibrium temperature of the water is 29.8C.
What is the final temperature of the metal?
C
What is the temperature change of the water?
C
What is the temperature change of the metal?
C
First, we need to calculate the heat gained by the water and the heat lost by the metal in order to determine the final temperature of the metal.
Using the formula:
q = mcΔT
where q is the heat gained or lost, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.
Assuming the specific heat capacity of water is 4.18 J/g°C and the specific heat capacity of the metal is 0.385 J/g°C, we can set up the following equation:
q_water = -q_metal
m_water * c_water * ΔT_water = - m_metal * c_metal * ΔT_metal
m_water * c_water * (T_f - T_i_water) = - m_metal * c_metal * (T_f - T_i_metal)
Let's calculate the final temperature of the metal:
70.4 - 29.8 = 40.6 (T_i_metal should be positive)
m_water * c_water * (29.8 - 23.6) = -m_metal * c_metal * (29.8 - 70.4)
(100g) * (4.18 J/g°C) * (6.2°C) = -(x) * (0.385 J/g°C) * (40.6°C)
2611.6 J = 40.6 * 0.385x
x = -6774.29 g
So the final temperature of the metal is -6774.29°C which is not possible.
The data given seems to be incorrect, or there may have been an error in the calculations.