m₁ = mass of sample of copper = m₂ = mass of sample of aluminum = 5 g
T = initial temperature of copper = initial temperature of aluminum
T₁ = final temperature of copper
T₂ = final temperature of aluminum
c₁ = specific heat of copper = 0.09 cal/g°C
c₂ = specific heat of aluminum = 0.22 cal/g°C
Since both receive same amount of heat, hence
Q₁ = Q₂
m₁ c₁ (T₁ - T) = m₂ c₂ (T₂ - T)
(5) (0.09) (T₁ - T) = (5) (0.22) (T₂ - T)
T₁ - T = (2.44) (T₂ - T)
Change in temperature of copper = (2.44) change in temperature of aluminum
hence the correct choice is
c. The copper will get hotter than the aluminum.
Answer: c. The copper will get hotter than the aluminum.
Explanation: Specific heat capacity of a substance is the amount of heat required to raise the temperature of 1 gram of water through [tex]1^0C[/tex]
As we know that,
[tex]Q=m\times c\times \Delta T[/tex]
m= mass
c = specific heat
[tex]\Delta T[/tex] = change in temperature
Given : [tex]Q_{Cu}=Q_{Al}[/tex]
mass of copper = mass of Aluminium= 5 g
[tex]c_{Cu}\times \Delta T_{Cu}=c_{Al}\times \Delta T_{Al}[/tex]
Now put all the given values , we get
[tex]0.09\times \Delta T_{Cu}=0.22\times \Delta T_{Al}[/tex]
Thus as specific heat capacity of copper is less, the temperature change will be more as they both are at same initial temperature.
