(Solved): A copper pot with mass 312kg is filled with 1.24L of water with which it is in equilibrium at a ...

A copper pot with mass $312\mathrm{kg}$ is filled with $1.24\mathrm{L}$ of water with which it is in equilibrium at a temperature of $20.3{}^{?}\mathrm{C}$. The pot of water is placed on a hot stove plate that transfers energy to the pot at a rate $P=24.0\mathrm{W}$ The specific heat capacity of copper is $c_{\text{copper }}=390\mathrm{J}?{\mathrm{kg}}^{?1}?{\mathrm{K}}^{?1}$ and that of water is $c_{\text{water }}=4186\mathrm{J}?{\mathrm{kg}}^{?1}?{\mathrm{K}}^{?1}$. Part 1) How much heat needs to be transferred to the system to bring the water to the boil? $Q=$ Part 2) How long will it take to bring the water to the boil? Ignore energy lost to the environment. $t=?\text{ seconds }$ Part 3) The pot with a lid on has an area of $0.88{\mathrm{m}}^2$ and has emissivity $e=0.85$. If the temperature of the room is $24.8^{?}\mathrm{C}$ calculate the initial net rate at which heat is transferred from the pot to the environment by thermal radiation. $P_{\mathrm{rad}}=?\mathrm{W}$