Answer:
Heat needed = 71.19 J
Explanation:
Here heat required can be calculated by the formula
H = mL
M is the mass of water and L is the latent heat of vaporization.
Mass of water, m = 31.5 g = 0.0315 kg
Latent heat of vaporization of water = 2260 kJ/kg
Substituting
H = mL = 0.0315 x 2260 = 71.19 kJ
Heat needed = 71.19 J
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.
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