Answer : The energy released will be, -11771.837 J
Solution :
Formula used :
\(Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})\)
where,
Q = heat released = ?
m = mass of copper = 28.9 g
c = specific heat of copper = \(0.385J/g^oC\)
\(\Delta T=\text{Change in temperature}\)
\(T_{final}\) = final temperature = \(25^oC\)
\(T_{initial}\) = initial temperature = \(1083^oC\)
Now put all the given values in the above formula, we get :
\(Q=28.9g\times 0.385J/g^oC\times (25-1083)^oC\)
\(Q=-11771.837J\)
Therefore, the energy released will be, -11771.837 J
