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flythisforme

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A 50g block of copper having a temperature of 400K is placed in an insulating box with a 100g block of lead having a temperature of 200K.

a) What is the equilibrium temperature of this two-block system?

b) What is the change in the internal energy of the two-block system as it goes from the initial condition to the equilibrium condition?

c) What is the change in the entropy of the two-block system?

I set the heat loss of the copper block equal to the heat gain of the lead block to find the equilibrium temperature using the equation deltaQ=mcdeltaT and got 318K as the answer for part (a). Is that correct?

Also, for part (b), would I find the change in internal energy of each block and add the two numbers together? Is there an equation to directly get changes in internal energy, or would I have to figure out the work first? (I know that deltaU = deltaQ - W)