Answer:
q = - 3.569KJ 0r 3.569KJ Liberated heat (signifying the change in heat is negative)
Explanation:
liberated heat implies that change in heat is negative , therefore
q = -m c ΔT
where, m = mass of the Silver = 249 g
c = specific heat capacity of Silver = 0.235 Jg^{-1} °C^{-1
ΔT = change in temperature = 87°C- 26 °C= 61°C
q = -m x c x ΔT
= - 249 x 0.235 x 61 = - 3569.415J rounded to -3569J
Changing to KJ becomes= -3569/1000= - 3.569 KJ
q = - 3.569KJ 0r 3.569KJ liberated heat.
