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A fertilizer (American English) or fertiliser (British English) is any material of natural or synthetic origin that is applied to soil or to plant tissues to supply plant nutrients. Fertilizers may be distinct from liming materials or other non-nutrient soil amendments. Many sources of fertilizer exist, both natural and industrially produced. [1]
Monopotassium phosphate (MKP) (also, potassium dihydrogen phosphate, KDP, or monobasic potassium phosphate) is the inorganic compound with the formula KH 2 PO 4. Together with dipotassium phosphate (K 2 HPO 4. (H 2 O) x) it is often used as a fertilizer, food additive, and buffering agent.
Most identities in chemical thermodynamics arise from application of the first and second laws of thermodynamics, particularly the law of conservation of energy, to these state functions. The three laws of thermodynamics (global, unspecific forms): 1. The energy of the universe is constant. 2.
Plant nutrition is the study of the chemical elements and compounds necessary for plant growth and reproduction, plant metabolism and their external supply. In its absence the plant is unable to complete a normal life cycle, or that the element is part of some essential plant constituent or metabolite .
The history of fertilizer has largely shaped political, economic, and social circumstances in their traditional uses. Subsequently, there has been a radical reshaping of environmental conditions following the development of chemically synthesized fertilizers .
Between the two types of the other compounds, Proust showed that no intermediate compounds exist between them. Proust published this paper in 1797, but the law was not accepted until 1812, when the Swedish chemist Jöns Jacob Berzelius gave him credit for it. [citation needed] There are, however, exceptions to the Law of Definite Proportions.
The second law determines whether a proposed physical or chemical process is forbidden or may occur spontaneously. For isolated systems , no energy is provided by the surroundings and the second law requires that the entropy of the system alone must increase: Δ S > 0.
The history of the Haber process begins with the invention of the Haber process at the dawn of the twentieth century. The process allows the economical fixation of atmospheric dinitrogen in the form of ammonia, which in turn allows for the industrial synthesis of various explosives and nitrogen fertilizers, and is probably the most important industrial process developed during the twentieth ...