Answer:
This is a question about calorimetry, which is the measurement of heat transfer between objects. To find the specific heat capacity of the metal, we need to use the principle of conservation of energy, which states that the heat lost by the metal is equal to the heat gained by the water. We can write this as:
Q_metal = -Q_water
where Q_metal is the heat transfer of the metal and Q_water is the heat transfer of the water.
We can also use the formula:
Q = mc∆T
where Q is the heat transfer, m is the mass, c is the specific heat capacity, and ∆T is the change in temperature.
Substituting these formulas into our equation, we get:
m_metal * c_metal * (∆T_metal) = -m_water * c_water * (∆T_water)
where m_metal and m_water are given as 21.5 g and 150.0 g respectively, c_water is known as 4.184 J/g°C, and ∆T_metal and ∆T_water can be calculated as:
∆T_metal = T_final - T_initial = 32.5°C - 98.0°C = -65.5°C ∆T_water = T_final - T_initial = 32.5°C - 23.5°C = 9°C
Plugging these values into our equation, we get:
21.5 * c_metal * (-65.5) = -(150) * (4.184) * (9)
Solving for c_metal, we get:
c_metal = (-(150) * (4.184) * (9)) / (21.5 * (-65.5)) c_metal ≈ 0.897 J/g°C
the value of specific heat capacity of metal in this experiment is approximately 0.897 J/g•°C.
Step-by-step explanation: