Answer : The energy needed is, [tex]7.55\times 10^{-3}kJ[/tex]
Explanation :
Formula used :
[tex]q=m\times c\times (T_{final}-T_{initial})[/tex]
where,
q = heat needed = ?
m = mass = 7.70 g
c = specific heat = [tex]0.140J/g^oC[/tex]
[tex]T_{final}[/tex] = final temperature = [tex]58^oC[/tex]
[tex]T_{initial}[/tex] = initial temperature = [tex]51^oC[/tex]
Now put all the given values in the above formula, we get:
[tex]q=7.70g\times 0.140J/g^oC\times (58-51)^oC[/tex]
[tex]q=7.546J=7.55\times 10^{-3}kJ[/tex]
Thus, the energy needed is, [tex]7.55\times 10^{-3}kJ[/tex]
