Solid honorite has a melting temperature of $261\mathrm{.}15K,$ and a heat capacity of $455\mathrm{.}4\frac{J}{k}gK.$ When it is liquid, its heat

capacity is $573\mathrm{.}4\frac{J}{k}gK.$ The latent heat for the transition from solid to liquid is $15300\frac{J}{k}g.$

Liquid odium has a freezing temperature of $328\mathrm{.}68K$ and a heat capacity of $434\mathrm{.}7\frac{J}{k}gK.$ When solid, its heat capacity is

$338\mathrm{.}7\frac{J}{k}gK.$ The latent heat for the transition from solid to liquid is $10800\frac{J}{k}g.$

A $4\mathrm{.}48kg$ block of honorite at $261\mathrm{.}15K$ is immersed in $13\mathrm{.}67kg$ of liquid odium at $390\mathrm{.}18K$ and left to achieve thermal

equilibrium in an isolated, insulated container.

How much energy was gained by the odium during this process? $($A positive value means energy was added. A negative

value means energy was lost.$)$

${10}^{4}J$