Answer:
Therefore, the highest final temperature is obtained in the container with Iron.
Explanation:
Q = mcΔT
Where;
Q is the quantity of heat gained or lost
m is the mass of the metals or water
c is the specific heat capacity
ΔT is the change in temperature, T₂ - T₁
T₂ is the final temperature and T₁ is the initial temperature
Heat lost by metals at 100°C is equal to heat gained by water at 25°C
[tex]-Q_{metal} = Q_{water}[/tex]
[tex]-Q_{Au} = Q_{H_2O} \\-Q_{Fe} = Q_{H_2O}[/tex]
Specific heat capacity of water = 4.18 J/g°C
Specific heat capacity of gold = 0.129 J/g°C
Specific heat capacity of iron = 0.45 J/g°C
⇒For Gold
-20*0.129*(T₂ - 100) = 18*4.18 (T₂ - 25)
-2.58T₂ +258 = 75.24T₂ - 1881
77.82T₂ = 2139
T₂ = 2139/77.82
T₂ = 27.49 ⁰C
⇒For Iron
-20*0.450*(T₂ - 100) = 18*4.18 (T₂ - 25)
-9T₂ +900 = 75.24T₂ - 1881
84.24T₂ = 2781
T₂ = 2781/84.24
T₂ = 33.01 ⁰C
Therefore, the highest final temperature is obtained in the container with Iron.
