# Question 77db3

Jun 1, 2017

$925 \text{ kJ}$ of heat is released.

#### Explanation:

The heat released is equal to the specific heat capacity, multiplied by the mass, multiplied by the temperature change:

Q=c*m*∆T

The specific heat capacity of water is $c = 4.18$ $\text{J"/"g˚C}$
This is how much energy it takes to heat one gram of water by one degree celsius (or how much heat is released upon cooling). In this case, the heat will be a negative value, as it is being released.

∆T=T_f-T_i=10.0-80.5=-70.5" ˚C"#

$m = 3140 \text{ g}$

$Q = 4.18 \cdot 3140 \cdot - 70.5 = - 925 \cdot {10}^{3} \text{ J}$

Therefore, $925 \text{ kJ}$ of heat is released.