Answer :
Answer:
[tex]Q=50,849.25J\\\\Q=12,153.3cal[/tex]
Explanation:
Hello!
In this case, given the mass, temperature change and specific heat, it is possible to compute the required heat in joules as shown below:
[tex]Q=mC(T_2-T_1)\\\\Q=75.0g*0.449\frac{J}{g\°C}(1535\°C-25\°C)\\\\Q=50,849.25J[/tex]
Now, since 1 cal =4.184 J, this result in calories is:
[tex]Q=50,849.25J*\frac{1cal}{4.184J}\\\\Q=12,153.3cal[/tex]
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