Problem: A 2.51 g lead weight, initially at 10.6˚C, is submerged in 7.86 g of water at 52.4˚C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium? (clead= 0.128 J/(g•oC))

FREE Expert Solution

$\overline{){\mathbf{q}}{\mathbf{=}}{\mathbf{mc}}{\mathbf{∆}}{\mathbf{T}}}$

+qabsorbs heat
–qloses heat

Heat transfer: hot to cold

heat released by water = heat absorbed by lead

At thermal equilibrium:

▪ final temperature of water = final temperature of lead = final temperature of system

Problem Details

A 2.51 g lead weight, initially at 10.6˚C, is submerged in 7.86 g of water at 52.4˚C in an insulated container. What is the final temperature of both the weight and the water at thermal equilibrium? (clead= 0.128 J/(g•oC))

What scientific concept do you need to know in order to solve this problem?

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