Nitrogen moles

TABLE III-25. ACTTION OF BENZOYL PEROXIDE ON 4-METHYLTHlAZOLE AT 80°C UNDER NITROGEN MOLE OF PEROXIDE/MOLE OF THIAZOLE) (184. 185)... 

Pn, = partial pressure of nitrogen Pnh3 = partial pressure of ammonia (-1 ) = rate of reaetion of nitrogen, moles of nitrogen disappearing per unit time per unit mass of eatalyst... 

Step 1 Determine nitrogen mole balance Inputs... 

Here, AH is in kJ - kg , MW is the molecular mass of the monomer xmit, m is the numbOT of moles of products formed in the stoichiometrically complete combustion of the polymer, and m is the number of nitrogen moles in the Oj/Nj atmosphere, per 1 mol of monomer unit. LOI is given as molar oxygen fraction in the atmosphere. 

After substituting Equations 3.1.2 and 3.1.3 into Equation 3.1.1, the oxygen mole balance reduces to Equation 3.1.4 in Table 3.1.1. Because Equation 3.1.4 is an unsteady-state, first-order differential equation, we need an initial condition to calculate the constant of integration. Initially, the tank contains air, which has an oxygen concentration of approximately 21 % by volume. We could also write the mole balance for nitrogen, but in this case it is more convenient to write the total mole balance, which results in Equation 3.1.5. Once we write Equations 3.1.4 to 3.1.6, the nitrogen mole balance is not an independent equation. Equation 3.1.7 states that the molar flow rate is equal to the product of the molar density and the volmnetric flow rate. 

First, drop all the repeated equations listed in Table 3.5.3. By substituting Equations 3.5.30 to 3.5.34 into Equations 3.5.19 to 3.5.22, we eliminate the mole fraction variables in line seven. We do not need Equations 3.5.35 to 3.5.39 for the solution, so they can be dropped. Table 3.5.2 lists the specified variables, except for the nitrogen mole fraction, y3 6, which is now unspecified. Table 3.5.7 lists the reduced set of equations. 

Pure methane is completely burned with air. The outlet gases from the burner, which contain no oxygen, are passed through a cooler, where some of the water is removed by condensation. The gases leaving the cooler have a nitrogen mole fraction of 0.8335. Calculate the following ... 

Let s consider a system that initially contains moles of nitrogen, moles of hydrogen, and... 

Z = moles of nitrogen/mole of oxygen in the TEG/air O = excess TEG/air ratio where 1 = zero oxygen in the products... 

We have tried to increase the reactivity of modified polystyrene by introducing sulphur bonds with small dissociation energy into its macromolecules. For that purpose we carried out styrene polymerization with tetramethylthiuram disulphide in the presence of sulfur as an initiator. The chemical composition of modified polystyrene was as follows 83.02% C, 7.28% H, 1.07% N, 7.91% S (Table 1). As acconsequence of the addition of sulfur to the reaction medium the sulfur/nitrogen mole ratio increased from 2 1 to above 3 1. The average molecula weight of po lystyrene modified by thiuram and sulfur was low, Mv = 2030 and = 2080. 

All of the above are gases except the solid with the empirical formula Ci()Hg. The gas stream (oxygen and nitrogen mole fractions of 0.01 and 0.099) is at 537.8°C with a Cp of 7.54 calories/g mole °K. Heat of combustion is —100 kilocalories per mole of oxygen consumed. If Sc is 0.8 and Pr 0.7, find the maximum possible particle temperature. 

Enzymes Activity per gm. wet weight (Mmoles/hour) Activity per mg. nitrogen ( moles/hour) ... 

Nitrogen Mole amounts may be quantitatively removed by reacting With titanium sponge, 14-20 mesh at 1000-1100 0. Use of lower temperatures (ca. 850 0) has been reported. Oxygen is also removed quantitatively. 

Thus 41.4% of the mixture is condensed with a nitrogen mole fraction in the condensate of 0.654 while the vapor in equilibrium with the condensate has a nitrogen mole fraction of 0.886. Note that the liquid and vapor concentrations agree with those shown in Fig. 6.9. 

Further cooling of the original mixture provides only a small enrichment of the nitrogen in the vapor. For example, immediately before total condensation of the mixture at a temperature of 78.9 K, the last trace of vapor will contain a nitrogen mole fraction of no better than 0.94. 

To complete the flash calculation, temperatures must be assumed until Eq. (6.25) is balanced (see Example 6.7). A temperature of 79.01 K satisfies the relation with a nitrogen vapor mole fraction of 0.930. With the aid of Eqs. (6.21) and (6.22) and Td = 79.51 K, we can now determine (following the procedure in Example 6.4) that the product stream leaving the top of the column has a nitrogen mole fraction of 0.908. This permits solution of the overall and component balance around the column represented by... 

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