Question 1182725
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Equal amounts of heat are added to equal masses of aluminum and iron at the same Initial temperature. 
Which metal will have the higher final temperature and how much greater will that temperature change be 
than the temperature change of the other metal
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To get the correct answer,  read the solution by  @Boreal and then turn it inside out.



&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<U>EXPLANATION</U>



<pre>
The specific heat of aluminum is  {{{S[a]}}} = 0.902 J/(g°C).


The specific heat of iron     is  {{{S[i]}}} = 0.450 J/(g*°C).


        (see this web-site  https://cpanhd.sitehost.iu.edu/C101webnotes/matter-and-energy/specificheat.html )



It means that you need 0.902 joules of heat to increase the temperature of one gram of aluminum by 1 °C,


and you need 0.450 joules of heat to increase the temperature of one gram of iron by 1 °C.


        The basic formula is  Q = S*m*dT,


where Q is the amount of heat (energy); S is the specific heat per gram of mass, m is the mass in grams; 
dT is increase (the change) of the temperature.


In this problem, we are given the same amount of heat energy (let say, 1 joule);
the same mass of two materials (let say, 1 gram);

so we have  

        dT = {{{1/S[a]}}} = {{{1/0.902}}} = 1.109 °C  for aluminum,

    and

        dT = {{{1/S[i]}}} = {{{1/0.450}}} = 2.222 °C  for iron.



So, the <U>ANSWER</U> is:  of the two materials, aluminum and iron, the iron will have more high temperature 

and the temperature change of IRON will be MORE THAN TWICE the temperature change of aluminum.
</pre>


One more time&nbsp;: &nbsp;&nbsp;the answer and the explanations in the post by &nbsp;@Boreal &nbsp;BOTH &nbsp;are incorrect.


The real and actual response of materials is &nbsp;OPPOSED &nbsp;to what &nbsp;@Boreal writes in his post.