Enthalpy
A datacenter rack is an exothermic system, in that air travelling into it produces a chemical reaction in which the system produces heat. Under conditions of constant pressure, the heat that is released is termed enthalpy (or "heat content").[SOURCE: Schmidt,IBM,2005]
bomb calorimeter measures heat transfer at constant while the cup measures at constant pressure.
Enthalpy
An isothermal process is one which does not take in or give off heat; it is perfectly insulated. Iso = same, thermal = heat. In real life there are very few isothermal processes. Heat loss accounts for most process inefficiencies.
I'm pretty sure its when the pressure remains constant. When the pressure is constant: q=delta U + P delta V The equation for delta H is: delta H = delta U +P delta V Therefore, when pressure is constant: delta H = q I think...
Yes it is possible, for example when water freezes there is a point when the temperature remains constant however energy is released as the water condenses.
A datacenter rack is an exothermic system, in that air travelling into it produces a chemical reaction in which the system produces heat. Under conditions of constant pressure, the heat that is released is termed enthalpy (or "heat content").[SOURCE: Schmidt,IBM,2005]
enthalpy, H
Heat of reaction.
Enthalpy-The heat added to or loss by a system at constant pressure
Heat of reaction.
This question is wrong. Heat capacity at constant pressure is more than that at constant volume. And Heat capacity at constant pressure - Heat capacity at constant volume= R Cp - Cv= R ,where R is universal gas constant.
In a closed system with constant pressure and no input or output of heat, the gas temperature will remain constant. In that same system, if the pressure is increased, then the gas temperature will also increase. If pressure is decreased, then the gas temperature will decrease.
The pressure is higher.
bomb calorimeter measures heat transfer at constant while the cup measures at constant pressure.
Enthalpy H is a thermodynamic state function, that is defined for homogeneous systems as H = U + P V where U is the internal energy of the system, P the pressure and V the volume. If we perform a transformation of the system between the states 0 and 1 maintaining the pressure constant, for the first thermodynamic principle, we have U1 - U0 = Q - P (V1 - V0) where Q is the heat the system absorbs during the transformation. From the definition of enthalpy we also have H1 - H0 = U1 - U0 + P (V1 - V0) Putting together the last two equations we get that, if pressure is maintained constant, H1 - H0 = Q that is the variation of enthalpy is equal too the heat absorbed during the transformation. Naturally this is not true if the pressure is not constant, but the case of constant pressure is particularly important since almost all chemical equations happen at constant pressure.
Yes it has! the specific heat of water at constant volume is given by cV : Heat capacity at constant volume cP : Heat capacity at constant pressure : Thermal expansion coefficient : Isothermal compressibility : Density