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高中化学课本第二册18—19页工业上制硝酸的原理是用氨氧化为一氧化氮,再氧化为二氧化氮,溶于水成硝酸和亚硝酸。困难的问题是氨的氧化要用催化剂,根据课本(19页图110)上介绍,在盛有氨水的烧杯里,用导管缓缓通入氧气,再用灼热的铂丝接近液面,周围就有白烟(NH_4NO_3),证明了一部分氨氧化为硝酸,又跟氨化合成硝酸铵。这个实验我们选用了四种催化剂,结果如下: (1)铁丝约一尺烧成螺旋状:插在玻棒一端,在喷灯上烧红,伸入盛有少量氨水的锥形烧瓶里,人概2—3次,则在液面有少量的白烟,证明铁丝可以供作氨氧化的催化剂,但效果差。
High School Chemistry Textbook Volume II, Pages 18-19 Industrial nitric acid is the principle of oxidation of ammonia to nitric oxide, then oxidized to nitrogen dioxide, dissolved in water into nitric acid and nitric acid. The difficulty is the use of ammonia oxidation catalyst, according to the textbook (Figure 110 on page 19) introduced in a beaker containing ammonia water slowly into the catheter with oxygen, then the hot platinum wire near the surface of the surrounding A white smoke (NH_4NO_3), proved that part of the ammonia oxidation to nitric acid, followed by ammonia synthesis of ammonium nitrate. This experiment we use four kinds of catalyst, the results are as follows: (1) about a foot of wire firing spiral: one end of the glass rod inserted in the torch burning red, into a conical flask containing a small amount of ammonia, 2-3 times, there is a small amount of white smoke in the liquid surface, which proves that iron wire can be used as a catalyst for ammonia oxidation, but the effect is poor.