The prime principal of the law of conservation of mass is that matter cannot be created nor destroyed. Although this is true during a chemical reaction, it is not always the case. This article explains that if matter and antimatter collide, both will be annihilated; and thus the matter is destroyed and its mass is transformed into energy.
This article explores how losing weight relates to the law of conservation of mass. Many people think that the mass they lose is just gone but that wouldn't make sense in terms of the law of conservation of mass. A team of Australian researchers found out what actually happens during the weight loss process. Most of the mass is exhaled as carbon dioxide while some is excreted as water through urine, tears, and sweat. This follows the law of conservation of mass.
This video talked about how the Law of Conservation of Mass was discovered. The person that founded the law was Antoine Lavoisier. He was expected to go into law but he chose science instead. Something that surprised me was that he married a 13 year old girl. He was beheaded in may 8 1794. The next contributor was a french pharmacist named Joseph Proust, he discovered the Law of Definite Proportions. After Proust was an english man named John Dalton confirmed the existence of atoms. We have these people and more after them to thank for the science we have today.
When you try to lose weight, where does it actually go? Does it break the law of conservation of mass? Hmm...
Some might say this is a contradiction, but it is not at all. "Losing" this matter is just process of the fat turning into carbon dioxide and water, which is released from your body via the lungs and urine, respectively. This article talks about the balance of how matter gained is released, and what actually happens when you gain or lose weight, and ALL explanations are following the law of conservation of mass.
This paper talks about how Antoine Laurent Lavoisier discovered the Law of Conservation of Mass around the year 1785. He made multiple experiments testing out his theory and he established that heat had nothing to do with the law. He realized that his results were as he predicted and so the Law of Conservation of Mass was established.
The law of conservation of mass states that matter cannot be created or destroyed. It is similar to when working with variables in math. In math, you can't just remove variables just from one side of the equation. you have to remove variables equally from both sides. For the law of conservation of mass, you must keep the amount of atoms for each element to be equal on the reactants side and the products side.
The Law of Conservation of Mass was created by Antoine Lavoisier in 1785. This led to the Law of Conservation of Energy created by Julius Robert Mayer and also the famous equation E=mc^2 by Albert Einstein. This famous equation only came to once it was discovered that all energy and mass in the universe is constant.
This article explains some of the implications of Einstein's famous equation, E=mc^2. One of those is the fact that in certain reactions, you can lose mass, seemingly breaking the law of conservation of mass. However, this is due to the fact that the mass is actually being converted to energy. In fact, 1kg of mass can be converted to 9x10^16 (90000000000000000) joules of energy. In comparision, on average, we only use about 5500000 joules a day! This conversion happens in many everyday reactions, such as radioactive decay, nuclear fission, or nuclear fusion.
This article explains that the first law of thermodynamics actually says that energy within a closed system cannot be created or destroyed. Later scientists discovered matter and energy are essentially equivalent. Therefore, the law of conservation of mass came to be.
During any physical or chemical change, the total mass of the products must be equal to the total mass of the reactants. If this is how we define the law of conservation of mass, then there are situations where it is violated.
In very energetic systems, like in nuclear reactions and particle-antiparticle annihilation, a certain part of the mass is converted into energy. This site redefines the law as: “during any physical or chemical change, the total mass of the products is equal to the total mass of reactants provided mass has not undergone conversion into energy,” which is much more specific and holds true through any change.
So many people obsess over diets and weight loss, yet only a few know how a kilogram of fat actually vanishes, a survey conducted with 150 doctors showed that 98% of them didn't know the right answer. The most common misconception was that fat is converted to energy. The problem with this theory is that it violates the law of conservation of mass. The correct answer is that fat is converted to carbon dioxide and water, you exhale the carbon dioxide and the water mixes into your circulation until it’s lost as urine or sweat.
The main idea of the law of Conservation of Mass is the that the same amount of of mass in the reactants will be the same amount in the products. This cartoon shows that although the number of minutes has been reduced by half, the population increased by double.
This article talks about the multiple meanings of Albert Einstein's famous equation, E=MC^2, and it's relation to the Law of Conservation of Mass. Simply put, masses at rest still have energy, mass can be converted into pure energy, and energy can be used to make mass out of nothing except pure energy.
The cartoon describes the law of conservation of mass in a funny situation. A man doesn't like his step mother, commenting that she was a mass that he didn't create or a mass he can destroy.
Even though the law of conservation of mass is said to be absolute, some chemical reactions seem to break the law because its products' weight is different than the reactants'. Antoine Lavoisier's experiments done in the 18th century, conducted in sealed glass jars, helped explain the occurrence.
For example, heating metal mercury would create a product that is heavier than the original metal. Lavoisier discovered that the total mass of the jar and the contents within had not changed themselves. He concluded that a gas in the air (oxygen) trapped in the jar must've reacted with mercury to form the product, making the product have both the mass of mercury and oxygen. Since the mass of the air was not accounted for the mass of the reactants, it created the illusion that new mass was created in the reaction. Lavoisier also came up with the conclusion that atoms cannot be created or destroyed in chemical reactions. Today in France, students are taught the law under the name "Lavoisier's Law" in honour of his contribution to discovering the principle.
This article explains the law of conservation of mass as well as its history. The idea of the total mass on earth being persistent was first proposed by the Ancient Greeks. Though, Antoine Lavoisier expressed the law of conservation of mass as a fundamental principle in physics in 1789. The law states that, regardless of chemical reactions or physical transformations mass is conserved. Meaning mass can not be created or destroyed in an isolated system; just rearranged. Basically, during a chemical reaction, the mass of the reactants will always be equal to the mass of the products. The law of conservation of mass is beneficial for a number of calculations. It may be used for solving unknown masses, for instance, calculating the amount of water produced during a chemical reaction.