The partial pressure of nitrogen

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 ... 

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 ( ). 

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.]... 

Niobium metal absorbs nitrogen, similar to hydrogen, forming interstitial solid solution. The absorption occurs at 300°C and the solubility of nitrogen in the metal is directly proportional to the square root of the partial pressure of nitrogen. The reaction is exothermic and the composition of such interstitial solid solution varies with the temperature. When the metal is heated with nitrogen at temperatures between 700 to 1,100°C, the product is niobium nitride, Nb2N or (NbNo.s) [12033-43-1]. When heated with ammonia at these temperatures, niobium forms this nitride. Another niobium nitride exists, NbN [24621-21-4], with a face-centered cubic crystalline structure. 

Another area in which the gas laws play a key role is in scuba diving. At the surface, we breath air at a pressure of approximately 1 atmosphere. The partial pressures of nitrogen and oxygen are 0.78 and 0.20 atmosphere, respectively. A scuba diver breaths compressed air that is delivered at a pressure that corresponds to the pressure at the depth of the diver. Because 33 feet of... 

Starting with a 10% nitrogen-in-helium mixture, the sample, held slightly above ambient pressure, is immersed in the coolant. When the adsorption signal is complete, the pressure is raised to 2 atm, which increases the partial pressure of nitrogen to 0.2 atm or the equivalent of a 20 % mixture at 1.0 atm. After the completion of each adsorption signal, the pressure is incrementally increased until, at ISOpsia saturation is reached. 

Consider the formation of ammonia from stoichiometric amounts of hydrogen and nitrogen in the gas phase (Eq. 9.4). If, after establishment of equilibrium, the total pressure is increased, does the partial pressure of nitrogen increase, decrease, or stay the same ... 

At 4000°K. the total vapor pressure of carbon is 0.43 atm. Consequently, the system is heterogeneous at 1 atm. pressure, and higher pressures can only be achieved by increasing the partial pressure of nitrogen. At pressures up... 

Self-Test 9.1A Calculate the change in molar free energy when the partial pressure of nitrogen in a mixture of gases is increased from 0.600 bar to 1.800 bar at 298 K. 

Stage 4 The balance between nitrogen dioxide and nitrogen tetroxide is calculated. This involves solution of a quadratic equation incorporating two reaction constants. The quadratic is shown below in terms of the partial pressure of nitrogen dioxide ... 

From a similar graph4 it is possible to calculate the partial pressure of nitrogen pentoxide, n2o6> at any time knowing the total pressure and the initial pressure. The pressure increase, P total — pi, 4 Details are given in J. Am. Chem. Soc., 43, 53 (1921). 

It was easy to control the partial pressure of nitrogen pentoxide by changing the temperatures of the crystals. When the crystals are placed in carbon dioxide snow at —80°, the partial pressure amounts to only about one one-hundredth of a millimeter. In this... 

The partial pressure of nitrogen pentoxide was maintained constant at 51.5 mm. in all the experiments. 

PROBLEM Refer to the example given above. Write an equation for the partial pressures of nitrogen and oxygen. If the total pressure in the container is 900 torr and the partial pressure of the oxygen gas is 560 torr, what is the partial pressure of the nitrogen gas ... 

How do the partial pressures of nitrogen gas and helium gas compare when a mole of nitrogen gas and a mole of helium gas are in the same closed container Refer to Table C-1 in Appendix C for a key to atom color conventions. 

What is the partial pressure of water vapor in an air sample when the total pressure is 1. (X) atm, the partial pressure of nitrogen is 0.79 atm, the partial pressure of oxygen is 0.20 atm, and the partial pressure of all other gases in air is 0.0044 atm ... 

A ternary B-N-O diagram was suggested to guide synthesis of hBN. Both appearance and structural ordering of reference amorphous boron in the production of hBN are highly dependent on the partial pressure of nitrogen . 

A is correct. The number of moles of gas is extra information. If the container began at 11 atm then each gas is contributing a pressure in accordance with its stoichiometric coefficient. When the reaction runs to completion, the only gas in the container is nitrogen dioxide, so the partial pressure of nitrogen dioxide is the total pressure. The volume of the container remains constant, so the pressure is in accordance with the stoichiometric coefficient of nitrogen dioxide. 

D is correct. You should know that 1 atm is equal to 760 torr. Since the partial pressure of nitrogen is 600, the mole fraction of nitrogen is 0.79. This means that the percentages given are by particle and not by mass. D would be true if the percentages were based on mass. If you chose B, you need to go back to Lecture 3 and review standard molar volume. 

The technique and the reaction system developed for the foregoing reaction was then applied to the study of a unimolecular reaction. The decomposition of nitrogen pentoxide has been found to remain unimolecular over enormous variations in pressure.12 But what is of most concern to the immediate problem is that it seems to remahji unaffected at extremely low pressures. Hunt and Daniels13 found that the decomposition rate was unchanged even when the partial pressure of nitrogen pentoxide... 

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