The heat of fusion for H 2 O at 273.15 K and 1 bar pressure is 6.008 kJ/mol; the heat of vaporization for H 2 O at 373.15 K and 1 bar pressure is 40.656 kJ/mol; and the molar heat capacity (C p,m) of liquid water between 273 K and 373 K has a nearly constant value of 75.29 J/K-mol (under a pressure of 1 bar).
It is expressed in units of energy (that is, the pressure-volume product) per kelvin per mole. It is equivalent to the Boltzmann constant, except that the latter is expressed in units of energy per kelvin per particle. Denoted by the symbol R, the value of the gas constant is: R = 8.314472 (15) J · K-1 · mol-1. An ideal gas has a gas constant R=0.4 kJ/kg-K and a constant-volume specific heat cu = 0.6 kJ/kg-K. If the gas has a temperature change of 90 °C. choose the correct answer for each of the following: The change in enthalpy is, in kJ/kg Select one: 30 70 OD 90 100The work done in expanding the gas is Q. One mole of an ideal gas expands at a constant temperature of $ 300K $ from an initial volume of $ 10 \,L $ to a final volume of $ 20 \,L $ .
Adiabatic expansion of a gas will lower its temperature; adiabatic compression of a gas will increase its temperature. 17.4.2. Constant Volume Processes. If the volume of a system is held constant, the system can do no work (W = 0 J). The first law of thermodynamics then shows that. ÆU = Q Oct 29, 2014 · ΔS sys = m(s 2 − s 1) = 2(1.9316 − 7.708) = −11.55 kJ/K The heat transfer to the surroundings occurs at constant temperature. Hence, the entropy change of the surroundings [see Eq.