# Question 8c237

Nov 17, 2016

It will take 764 kJ of heat energy.

The energy $q$ required to heat an object is given by the formula

color(blue)(bar(ul(|color(white)(a/a)q = mcΔTcolor(white)(a/a)|)))" "

where

$m$ is the mass
$c$ is the specific heat capacity
ΔT is the change in temperature

$m = \text{2.60 kg" = "2600 g}$
$c = \text{1.75 J·°C"^"-1""g"^"-1}$
ΔT = T_"f" - T_"i" = "191 °C - 23 °C = 168 °C"
q = 2600 color(red)(cancel(color(black)("g"))) × "1.75 J"·color(red)(cancel(color(black)("°C"^"-1"·"g"^"-1"))) × 168 color(red)(cancel(color(black)("°C"))) = "764 400 J" = "764 kJ"#