Navigating the world of chemistry is much easier once you understand the basic laws of the field. Here are brief summaries of the laws, basic concepts, and most important principles of chemistry: Since matter cannot be produced or destroyed, we must have four hydrogens and two oxygens on either side of the equation – on both sides of the chemical reaction. Chemistry is the science that studies matter, its structure, formation and the transformations it undergoes, taking into account the energy involved in the whole process. In ancient Greece, philosophers like Aristotle were already interested in knowing what matter was made of and how its transformations occurred. Today, we know that, unlike Aristotle, matter is not made up of the essential substances of water, fire, earth and air. However, his philosophical work in questioning the origin of matter formed the basis for the discussion of chemical elements and their combinations. Before examining explicit examples of the law of conservation of matter, we must examine the method used by chemists to represent chemical changes. What does this mean for chemistry? With each chemical change, one or more raw materials are converted into one or more other substances. The starting and ending substances are made up of atoms, since all matter is composed of atoms. According to the law of conservation of matter, matter is neither created nor destroyed, so after the chemical change, we must have the same number and type of atoms that were present before the chemical change. Express the law of preservation of matter in your own words. Explain why the concept of preserving matter is considered a scientific law. The Law on Energy Saving is the first fundamental law concerning a thermodynamic system.
Julius Robert Mayer discovered the law of conservation of energy. The law states that: The idea of preserving the mass already had philosophical references in ancient Greece. The idea at that time was that matter could not be created or destroyed from anything, but already existed and could be transformed. For example, if 2 grams of hydrogen react with 16 grams of oxygen, 18 grams of water are produced; When 12 grams of carbon react with 32 grams of oxygen, 44 grams of carbon dioxide are produced. Law of preservation of mass = matter is neither created nor destroyed. This law is attributed to Lavoisier (1743-1794). A scientific law that forms the basis of understanding in chemistry is the law of the preservation of matter. It states that in any given closed system for the transfer of matter (pure and output), the amount of matter in the system remains constant. A succinct way to express this law is to say that the amount of matter in a system is preserved. Any change in the magnetic environment of a wire coil causes a voltage (CEM) to be “induced” in the coil. No matter how the change is generated, the tension is generated.
This is clearly stated by Faraday`s law. The law of mass conservation follows the laws of matter and can be described by balanced chemical equations. In this case, balancing a chemical equation means ensuring that the atoms present in the equation are in the same number in the reactants and products. Therefore, unbalanced chemical equations do not effectively demonstrate the law of mass conservation because the number of atoms in reactants is not the same as in products. As an example, we can consider the equation of water formation. His unbalanced equation can be seen below:. So let`s go through a chemical and nuclear reaction to show how the mass before a reaction corresponds to the mass after a reaction. Many examples of chemical combinations can be found in everyday life. For example, the combination of oxygen and hydrogen gases in water.
Another example is the formation of rust or iron oxide from the combination of iron atoms with gaseous oxygen molecules. The coefficient before HBr balances the equation of mass. The law of certain proportions = a given compound always contains exactly the same proportion (ratio) of the elements in mass. One of the founders of atomic theory, the English chemist John Dalton, also studied the masses of reactants and products and contributed to chemical laws. To formulate the theory of multiple proportions, he discovered that as soon as a solid mass of an element connects to different masses of a second, it ends up creating different connections. For example, if you consider the formation of nitrogen oxides from nitrogen gas and gaseous oxygen:. My blog only gives you the first 3 videos of each of the 20 sections (chapters). Example: Consider the decomposition of water into its elements. The law of constant proportions, also known as the law of certain proportions, is one of the chemical laws and was developed in 1797 by the chemist Joseph Louis Proust.
He found that the masses of reactants and the masses of products involved in a chemical reaction always obey a constant ratio. This proportion is characteristic of each reaction and regardless of the number of substances introduced into the reaction. So let`s look at the formation of copper sulfide (CuS) by copper (Cu) and sulfur (S): now we remove sulfur from each ratio to give us the hydrogen/oxygen ratio, which is 1 H:1 O. Show how this data illustrates the law of multiple proportions. A chemical combination is a phenomenon that describes the interaction between chemical substances and new substances. Chemical combinations can be represented by the equations of the chemical reactions they represent. In this sense, chemical combinations are subject to the chemical laws of reactions. These laws are: For example, carbon dioxide always has the ratio of one carbon atom to two oxygen atoms, which leads to the formula CO2. The mass ratio is also constant: 12 g of carbon to 32 g of oxygen, which are rounded figures from the periodic table. The law of multiple proportions is as follows. These are just a few of the many laws of chemistry that everyone should understand.