Nitrogen molar heat capacity

A sample of nitrogen gas of volume 20.0 L at 5.00 kPa is heated from 20.°C to 400.°C at constant volume. What is the change in the entropy of the nitrogen The molar heat capacity of nitrogen at constant volume, CVm, is 20.81 J-K -mol . Assume ideal behavior. 

The heat capacity of thiazole was determined by adiabatic calorimetry from 5 to 340°K by Goursot and Westrum (295,296). A glass-type transition occurs between 145 and 175 K. Melting occurs at 239.53°K (-33.62°C) with an enthalpy increment of 2292 cal mole" and an entropy increment of 9.57 cal mole" -"K". Table 1-44 summarizes the variations as a function of temperature of the most important thermodynamic properties of thiazole molar heat capacity Cp, standard entropy S°, and Gibbs function -(G°-The variation of Cp for crystalline thiazole between 145 and 175°K reveals a marked inflection that has been attributed to a gain in molecular freedom within the crystal lattice. The heat capacity of the liquid phase varies nearly linearly with temperature to 310°K, at which temperature it rises more rapidly. This thermal behavior, which is not uncommon for nitrogen compounds, has been attributed to weak intermolecular association. The remarkable agreement of the third-law ideal-gas entropy at... 

Problem From the data in Tables II and IV estimate the variation of the molar heat capacity of nitrogen with pressure, at ordinary temperatures and pressures. 

Calculate the molar heat capacity at 1 atm. pressure of nitrogen at 0 , 600 and 1000 C. Compare the results with the mean heat capacity in the range from 0 to 1000 C. 

Fig. 9,7, The molar heat capacity at constant volume of diatomic gases hydrogen, x nitrogen, O iodine.

The molar heat capacity of a diatomic molecule is 29.1 J/K mol. Assuming the atmosphere contains only nitrogen gas and there is no heat loss, calculate the total heat intake (in kilojoules) if the atmosphere warms up by 3°C during the next 50 years. Given that there are 1.8 X 10 ° moles of diatomic molecules present, how many kilograms of ice (at the North and South Poles) will this quantity of heat melt at 0°C (The molar heat of fusion of ice is 6.01 kJ/mol.)... 

The molar heat capacity of a diatomic molecule is 29.1 J/K mol. Assuming the atmosphere contains only nitrogen gas and there... 

What is the change in molar enthalpy of N2 when it is heated from 25.0 °C to 100.0 °C The molar heat capacity of nitrogen is given by... 

The first coefficient describes the most common case, namely how much entropy AS flows in if the temperature outside and (also inside as a result of entropy flowing in) is raised by AT and the pressure p and extent of the reaction are kept constant. In the case of the secmid coefficient, volume is maintained instead of pressure (this only works well if there is a gas in the system). In the case of J = 0, the third coefficient characterizes the increase of entropy during equilibrium, for example when heating nitrogen dioxide (NO2) (see also Experiment 9.3) or acetic acid vapor (CH3COOH) (both are gases where a portion of the molecules are dimers). Multiplied by T, the coefficients represent heat capacities (the isobaric Cp at constant pressure, the isochoric Cy at constant volume, etc.). It is customary to relate the coefficients to the size of the system, possibly the mass or the amount of substance. The corresponding values are then presented in tables. In the case above, they would be tabulated as specific (mass related) or molar (related to amount of substance) heat capacities. The qualifier isobaric and the index p will... 

Problem Find the molar enthalpy of reaction for the standard state formation of ammonia from hydrogen and nitrogen at 298, 400, 600, and 800 K (1) assuming constant heat capacities for reactants and products and (2) using 29.75 + 0.025T - 150,000/7 for the heat capacity (J mol ) of ammonia. 

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