Question

A 2.84 g lead weight, initially at 10.6 ∘C, is submerged in 7.68 g of water at 52.6 ∘C in an insulated container. What will be the final temperature of the system when thermal equilibrium is reached?

A) 31.6 ∘C
B) 32.8 ∘C
C) 42.1 ∘C
D) 46.5 ∘C

Answer 1

The question pertains to calculating the final temperature of a lead weight and water when they reach thermal equilibrium in an insulated container, which is resolved by applying the principles of calorimetry and solving the corresponding heat transfer equations.

Step-by-step explanation:

The question is about finding the final temperature of a system consisting of a lead weight and water when they reach thermal equilibrium. This is a classic calorimetry problem involving heat transfer between two substances, which means we'll apply the concept that the heat lost by the lead will be equal to the heat gained by the water. To find the final temperature, we use the formula:

Qlost = Qgained

mPb × cPb × (ΔT)Pb = mH2O × cH2O × (ΔT)H2O

Where m is the mass, c is the specific heat capacity, and ΔT is the change in temperature.

By plugging in the known values and solving for the final temperature, Tfinal, we can find the temperature at which the system will be in equilibrium. Remember that the specific heat capacity of water (cH2O) is typically accepted as 4.18 Joules per gram per degree Celsius (J/g°C) and the specific heat capacity of lead (cPb) is approximately 0.128 J/g°C.