Question

A molten sample of 1.00kg of iron with a specific heat of 0.385J/g.K at 1000.K is immersed in a sample of water. If the water absorbs 270 kJ of heat what is the final temperature of the iron?

I need all the process.

Answer 1

298. 7 K.

Step-by-step explanation:

Hello!

In this case, since equation we use to compute the heat in a cooling or heating process is:

`Q=mC(T_f-T_i)`

Whereas we are given the heat, mass, specific heat and initial temperature. Thus, we infer that we need to solve for the final temperature just as shown below:

`T_f=T_i+(Q)/(mC)\\\\T_f=1000 K+(-270000J)/(1000g*0.385(J)/(g*K) ) \\\\T_f=298.7 K`

It is important to notice that the iron release heat as water absorbs it, that is why it is taken negative.

Best regards!