How was liquid nitrogen invented?
Nitrogen was first liquefied on April 15, 1883 at Jagiellonian University by Polish physicists Zygmunt Wr_Blewski and Karol Olszewski. Read more exciting novels for free
Is liquid nitrogen gas or liquid?
Liquid nitrogen was a liquid, and its English name was Liquid nitrogen. It was the liquid form of nitrogen (N2). It was a colorless, transparent, odorless, and extremely cold liquid that was slightly dissolved in water and easy to flow. The novel "Watching the Moon on Fish Island" is equally exciting. Everyone is welcome to click and read it!
Molar nitrogen and nitrogen react?
Under certain conditions, the reaction between nitrogen and nitrogen can occur. For example, in the presence of oxygen, the reaction between nitrogen and nitrogen can produce nitrogen.(4NH2 + 3O2 = ignition = 2N2 + 6H2 O); The synthetic nitrogen reaction is the reaction of nitrogen and hydrogen to produce nitrogen gas (N2 + 3H2 2NH2, catalyst, high temperature and high pressure). This is a irreversible reaction. From the reverse process of this reaction, nitrogen gas can also be converted to nitrogen and hydrogen under certain conditions; The reaction of nitrogen dioxide and nitrogen gas can produce nitrogen and water (4NH3 + 6NO = 5N2 + 6H2O). However, if it was simply a reaction between nitrogen and nitrogen, they would not react under normal circumstances. This was because nitrogen was a very inactive chemical gas that did not easily react with other substances. As for the discussion on this issue on Zhihu, he could not tell them exactly because he did not find any relevant content. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Absorbency of blank value of nitrogen and nitrogen
In the detection of nitrogen and nitrogen, the blank light absorption referred to the light absorption obtained by measuring the light source, the cuvette, and other optical systems without any sample. The blank absorption range of nitrogen nitrogen was a key factor in the process of nitrogen nitrogen detection. It played an important role in ensuring the accuracy and reliability of the test results. The reagent blank for the determination of nitrogen and nitrogen shall have an absorption value of not more than 0.030 (10mm cuvette), and the test water blank shall have an absorption value of not more than 0.030 to meet the requirements of determining the absence of nitrogen and nitrogen. "Little Fox Fairy" is equally exciting. Everyone is welcome to click and read it!
Nessler's reagent standard curve for determining nitrogen nitrogen
The following is the content related to the standard curve of Nessler's reagent for determining nitrogen and nitrogen: 1. ** Steps of Drawing the Calibrating Curv ** - Add 0.00, 0.50, 1.00, 2.00, 4.00, 6.00, 8.00, and 10.00ml of the standard working solution of nitrogen into eight 50ml color comparison tubes, respectively. The corresponding contents of the standard working solution of nitrogen and nitrogen are 0.0, 5.0, 10.0, 20.0, 40.0, 60.0, 80.0, and 100.0 ug, respectively. Add water to the marking line. - Add 1.0ml of the solution of potassium-Na tartrate and shake it well. Then add 1.5ml of mercuric chloride-potassium iodide-potassiumoh solution or 1.0ml of mercuric iodide-potassium iodide-potassiumoh solution (Nessler's reagent) and shake it well. - After standing for 10 minutes, measure the absorption with a 20-mm light path cuvette at a wave length of 420 mm and water as a reference. - The absorption after blank correction was used as the ordinate and the corresponding nitrogen content (ug) was used as the abyssal coordinate to draw the correction curve. A 10mm cuvette can also be used according to the mass concentration of the sample to be tested. 2. ** Exemplary Data ** - For example, some data showed that when the nitrogen content was 0.000g, the light absorption was 0.028, and when the nitrogen content was 0.005g, the light absorption was 0.055. A standard curve was drawn based on these data points (the content of nitrogen and its corresponding light absorption). For example, the data was as follows: - No. 1: Volume: 0ml, standard concentration of nitrogen nitrogen: 10 ug/ml (mass: 0 ug), absorption value: 0.096. - No. 2: Volume: 1ml, standard concentration of nitrogen nitrogen: 10 ug/ml (mass: 10 ug), light absorption value: 0.14. - Number 3: The volume is 2ml, the standard concentration of nitrogen is 10 ug/ml (mass is 20 ug), and the absorption value is 0.179. According to these data, a standard curve of the relationship between the nitrogen content and the light absorption can be drawn. This curve is generally linear, for example, it meets the linear equation of <y = 3.512x+ 0.0048>(where <y> is the corrected light absorption, and <x> is the nitrogen content), which is used to calculate the nitrogen content according to the measured light absorption. "Little Fox Fairy" is equally exciting. Everyone is welcome to click and read it!
What will happen to the reaction of iron sulfuric acid and nitrogen nitrogen?
Based on context alone Iron Sulphate (Fe2 (SO)) and nitrogen nitrogen (usually in the form of NHin solution) will react. In the solution, iron ions (Fe3) will be produced by the dissolution of iron sulfuric acid, and the iron ions will undergo a double decomposition reaction with the lithium ions (NH3). Iron ions were decomposed to produce iron (III), while the nitrogen ions were decomposed to produce nitrogen (III). The nitrogen ions were unstable and would decompose to produce nitrogen (III). The reaction equation was roughly as follows: Fe₂(SO₄)₃ + 6NH₄⁺ + 6H₂O = 2Fe(OH)₃↓+ 3(NH₄)₂SO₄ + 6H⁺ (NH The reaction will continue to proceed to the right, and the nitrogen ions will be further decomposed to produce hydrogen gas that escapes from the system. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
How to test for nitrogen?
The test method for the colorless and pungent odor of the gas was as follows: First, it could be tested with a wet red litmus test paper. If the test paper turned blue, it proved the existence of the gas. Second, a glass rod dipped in concentrated sulfuric acid was used to approach the gas to be tested. If white smoke was produced, it indicated the existence of the gas. While waiting for the TV series, you can also click on the link below to read the classic original work of "Dafeng Nightwatchman"!
Reaction of nitrogen and ethene
Under high temperature and high pressure and with a catalyst, ethene and nitrogen can react to form Pyrazine (C2H4N2) and hydrogen (H2). During this process, the carbon atoms of ethene combine with the nitrogen atoms of nitrogen to form new compounds. However, there was also a view that nitrogen was very stable and usually did not react with ethene. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
Reaction of silver and nitrogen
The solution of silver amine was the solution of AgNOH. When it was mixed with the solution of NaOx, the solution of NaOx would cause the balance of the solution of silver amine to shift to the right, forming silver solute. The silver solute would decompose into silver dioxide under the light. The reaction process was (AgNOH) NOH = AgNOH → 2NOH. <a href="/?from=ask_words" style="color:red" target="_blank">Read more exciting novels for free</a>
There is color in the blank when the Nessler reagent is used to measure the nitrogen nitrogen.
There may be the following reasons for the color of the blank in the Nessler's reagent: 1. ** The characteristics of the Nessler's reagent itself **: The Nessler's reagent is a slightly yellowish green transparent solution at room temperature. As the exposure time increases, it will gradually form a yellowish brown deposit, and the solution will gradually turn yellow. If the exposure time of the Nessler's reagent in the blank experiment was too long, it might cause color to appear. 2. ** Experiment operation factors ** - ** Cuvette problem **: If a 1cm cuvette is used, the blank value of the blank absorption is too high and is greater than 0.030, which may cause color to be seen. The first reason was the purity of the reagent, such as the reagent used containing an aminium salt (such as potassium-Na tartarate); the second reason was that the test water was contaminated and the introduction of an aminium salt. - ** Inappropriate use of Nessler's reagent **: Nessler's reagent needs to be kept at room temperature before use, and it cannot be shaken before use. It should be used by absorbing the supernate. If this operation is not followed, the blank color may be affected. 3. ** Purity and contamination of reagents ** - [** Impurity in the reagent **: The order of adding the medicine in the preparation of the Nessler's reagent is different, and the phenomenon of different colors often occurs.] - ** Contained **: If the experimental water or other reagents are contaminated with either nitrogen or nitrogen, the Nessler's reagent will also produce a color reaction in the blank experiment. "Little Fox Fairy" is equally exciting. Everyone is welcome to click and read it!
There is a red deposit when the Nessler's reagent is added to the nitrogen nitrogen.
If there was a red deposit in the water sample after adding Nessler's reagent, it might be because the water sample was acidic. According to the relevant standards, the Nessler's reagent method should be used to determine the nitrogen nitrogen in the basic solution. If the water sample was fixed with acid, the Nessler's reagent would be added directly without adjusting the ph to the appropriate range (6 - 9) during the measurement. The acidic environment of the water sample would cause red precipitations, which would affect the measurement results. In this case, the result of the test with a thermometer may be zero or the reagent blank value. This was because the components in the Nessler's reagent would normally react with nitrogen to form a reddish brown complex for determining the content of nitrogen and nitrogen under acidic conditions. "Little Fox Fairy" is equally exciting. Everyone is welcome to click and read it!