In summer the atmospheric temperature goes higher than our body temperature that is 37 degrees celsius. To maintain our body temperature fixed at 37 degrees our body looses heat.
The specific heat capacity of water is 4.18 J/g/°C. We wish to determine the value of Q - the quantity of heat. To do so, we would use the equation Q = m•C•ΔT. The m and the C are known; the ΔT can be determined from the initial and final temperature.Specific heat capacity is defined as the amount of heat required to raise the temperature of 1 kilogram of a substance by 1 kelvin (SI unit of specific heat capacity J kg−1 K−1).
For liquid at room temperature and pressure, the value of specific heat capacity (Cp) is approximately 4.2 J/g°C. This implies that it takes 4.2 joules of energy to raise 1 gram of water by 1 degree Celsius.In a system, Cp is the amount of heat energy released or absorbed by a unit mass of the substance with the change in temperature at a constant pressure. ... So, Cp represents the molar heat capacity, C when pressure is constant. The change in temperature will always cause a change in the enthalpy of the system.
Molar heat capacity is a measure of the amount of heat necessary to raise the temperature of one mole of a pure substance by one degree K. Specific heat capacity is a measure of the amount of heat necessary to raise the temperature of one gram of a pure substance by one degree K.Our body is constantly producing heat – our muscles, many chemical reactions work to make heat. This heat increases our core body temperature and one way in which our body dissipates this heat is by sweating. ... And so, in response, our bodies sweat more in summer.
When the weather is hot or your body temperature rises due to exercise or fever, sweat is released through ducts in your skin. It moistens the surface of your body and cools you down as it evaporates.