Pressure of nitrogen

A positive pressure of nitrogen is maintained using a mercury bubbler. 

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... 

A dry, 500-ml, three-necked flask is fitted with a mechanical stirrer, a condenser, and a pressure-equalizing dropping funnel. The system is swept out with nitrogen and a slight positive pressure of nitrogen is maintained by venting the system to a mercury filled U-tube. In the flask is placed 21 g (0.187 mole) of dry potassium /-butoxide, and the flask is cooled in an ice-salt bath. 

A sample of nitrogen is collected over water at 18.5°C. The vapor pressure of water at 18.5°C is 16 mm. When the pressure on the sample has been equalized against atmospheric pressure, 756 mm, what is the partial pressure of nitrogen What will be the partial pressure of nitrogen if the volume is reduced by a factor 740/760 ... 

Let us examine a chemical reaction to see if these same conditions apply. Suppose we fill two identical bulbs to equal pressures of nitrogen dioxide. Now immerse the first bulb (bulb A) in an ice bath and the second bulb (bulb B) in boiling water, as in Figure 9-4. The gas in bulb A at 0°C is almost colorless the gas in bulb B at 100°C is reddish-brown. The predominant molecular species in the cold bulb must be different from that in the hot bulb. A variety of experiments shows that the cold bulb contains mostly N204 molecules. These same experiments show that the hot bulb contains mostly NOa molecules. The N20 molecules absorb no visible light, so... 

Self-Test 9.9A The initial partial pressures of nitrogen and hydrogen in a rigid, sealed vessel are 0.010 and 0.020 bar, respectively. The mixture is heated to a temperature at which K = 0.11 for N2(g) + 3 H2(g) 2 NH3(g). What are the equilibrium partial pressures of each substance in the reaction mixture ... 

Now let s discuss the pressure computations. The observed reactor pressure is a sum of the partial pressures of nitrogen and the styrene monomer vapor. The vapor pressure of the styrene vapor is an increasing function of temperature and decreasing function of conversion. This is explained by the Flory-Huggins relationship ( ). 

Nitrogen is introduced via a syringe needle that pierces the septum. A positive pressure of nitrogen is maintained in the apparatus during the following operations. 

The oxide is used to effect rapid decomposition of hydrazine in a high-temperature gas generator which produces exit pressures (of nitrogen, hydrogen and ammonia) of 550 bar. 

A very attractive method for the preparation of nitroalkenes, which is based on the reaction with NO, has been reported. Treatment of alkenes at ambient pressure of nitrogen monoxide (NO) at room temperature gives the corresponding nitroalkenes in fairly good yields along with P-nitroalcohols in a ratio of about 8 to 2. The nitroalcohol by-products are converted into the desired nitroalkenes by dehydration with acidic alumina in high total yield. This simple and convenient nitration procedure is applied successfully to the preparation of nitroalkenes derived from various terminal alkenes or styrenes (Eq. 2.27).53 This process is modified by the use of HY-zeolites instead of alumina. The lack of corrosiveness and the ability to regenerate and reuse the catalyst make this an attractive system (Eq. 2.28).54... 

Fig. 4.2 Comparison of amino acid yields using CH4, CO and CO2 as carbon sources with the addition of varying amounts of H2. The yields were calculated on the basis of the amount of carbon present in the reaction mixture. In all cases, the partial pressures of nitrogen, methane, carbon monoxide and carbon dioxide were lOOmmHg. For the reactions using nitrogen, the reaction vessel contained 100 mL of water, but no ammonia. Reactions involving nitrogen and ammonia were carried out using 100 mL of ammonium chloride (0.05 M). The electrical discharge experiments took 48 hours at room temperature (Schlesinger and Miller, 1983)...

Plan (1) Calculate the partial pressure of nitrogen in the container at 25°C and 750. torr. 

SAQ 5.7 What is the total pressure of 10 g of nitrogen gas and 15 g of methane at 298 K, and what is the partial pressure of nitrogen in the mixture [Hint you must first calculate the number of moles involved.]... 

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