Respuesta :
Explanation:
(a). The given data is as follows.
Volume of one glass of water = [tex]2.2 \times 10^{2}[/tex] ml = 220 ml
Volume of 4 glass of water = [tex]220 \times 4[/tex] = 880 ml
We known that density of water is 1 g/ml. Therefore, calculate the mass of water as follows.
Mass of water = [tex]880 ml \times 1 g/ml[/tex]
= 880 gm
= 0.88 Kg (as 1 kg = 1000 g)
The relation between heat energy, mass and temperature change is as follows.
Q = [tex]mC \Delta T[/tex]
[tex]\Delta T = (37 - 3.2)^{o}C = 33.8^{o}C[/tex]
Putting the given values into the above formula as follows.
Q = [tex]mC \Delta T[/tex]
= [tex]0.88 \times 4.186 J/g^{o}C \times 33.8^{o}C[/tex]
= 124.5 kJ
Hence, the body have to supply 124.5 kJ to raise the temperature of the water to 37 degree C.
(b). As we know that the heat of fusion of ice is 333 J/g.
So, energy required for [tex]8.4 \times 10^{2}[/tex] g or 840 g is as follows.
[tex]333 \times 840[/tex] = 279.72 kJ
Heat capacity of water= 4.184 [tex]J/g^{o}C[/tex]
Now, heat energy will be as follows.
Q = [tex]4.184 \times 840 g \times 37^{o}C[/tex]
= 130.03 kJ
Therefore, total heat required = (279.72 + 130.03) kJ
= 409.75 kJ
Hence, for the given situation your body should lose 409.75 kJ of heat.
