Question

How much heat energy, in joules, is released to your body after you drink a cup of hot tea containing 125g of water that is cooled from 55℃ to a body temperature at 37℃ (water has a specific heat capacity of 4.184 J/g℃

Answer 1

`Q=-9414J`

Step-by-step explanation:

Hello,

In this case, the released heat by the water in this heating process is defined in terms of its mass, heat capacity and temperature difference as shown below:

`Q=mCp\Delta T`

Thus, with the given data indicating that water was at 55 °C before entering the body, we obtain:

`Q=125g*4.184(J)/(g^oC)*(37-55)^oC`

`Q=-9414J`

Such negative result means that the water releases that amount of heat to the body.

Best regards.

Answer 2

`Q_(out) = 9414\,J`

Step-by-step explanation:

The heat release to the human body is determined with the help of the First Law of Thermodynamics:

`-Q_(out) + U_(in) - U_(out) = 0`

`Q_(out) = U_(out) - U_(in)`

`Q_(out) = m\cdot c_(w)\cdot \Delta T`

`Q_(out) = (125\,g)\cdot \left(4.184\,(J)/(g\cdot ^(\textdegree)C) \right)\cdot (55^(\circ)C - 37^(\circ)C)`

`Q_(out) = 9414\,J`