A metal bar having a mass of 212 g is heated to 125.0°C and then dropped into 375 g of water at 24°C. After a while the temperature of the water and the metal is 34.2°C. If the specific heat of the metal is 0.831 J/g°C, how much heat did the metal lose?
q lost by metal = mass metal x specific heat metal x (Tfinal-Tinitial) = ?
Thank you so much!!
To calculate the amount of heat lost by the metal, we need to use the equation:
Q = mcΔT
Where:
Q is the heat lost by the metal
m is the mass of the metal
c is the specific heat of the metal
ΔT is the change in temperature
We are given:
m (mass of the metal) = 212 g
c (specific heat of the metal) = 0.831 J/g°C
To find ΔT, we need to calculate the change in temperature for both the metal and the water. The ΔT for the metal can be calculated as the final temperature minus the initial temperature, so:
ΔTmetal = 34.2°C - 125.0°C = -90.8°C
Now we can calculate the heat lost by the metal using the equation mentioned above:
Q = mcΔT
= (212 g) × (0.831 J/g°C) × (-90.8°C)
= -16108.472 J
Therefore, the metal lost approximately 16,108.472 J of heat.