John dalton experimental design
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John Dalton
Modern Atomic Theory (John Dalton)
Experiments with gases that first became possible at the turn of the nineteenth century led John Dalton in to propose a modern theory of the atom based on the following assumptions.
1. Matter is made up of atoms that are indivisible and indestructible.
2. All atoms of an element are identical.
3. Atoms of different elements have different weights and different chemical properties.
4. Atoms of different elements combine in simple whole numbers to form compounds.
5. Atoms cannot be created or destroyed. When a compound decomposes, the atoms are recovered unchanged.
Dalton's Law of Partial Pressures (John Dalton)
John Dalton was the first to recognize that the total pressure of a mixture of gases is the sum of the contributions of the individual components of the mixture. By convention, the part of the total pressure of a mixture that results from one component is called the partial pressure of that component. Dalto
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John Dalton
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Who Was John Dalton?
During John Dalton's early career, he identified the hereditary nature of red-green color blindness. In he revealed the concept of Dalton’s Law of Partial Pressures. Also in the s, he was the first scientist to explain the behavior of atoms in terms of the measurement of weight.
Early Life and Career
Dalton was born in Eaglesfield, England, on September 6, , to a Quaker family. He had two surviving siblings. Both he and his brother were born color-blind. Dalton's father earned a modest income as a handloom weaver. As a child, Dalton longed for formal education, but his family was very poor. It was klar that he would need to help out with the family finances from a ung age.
After attending a Quaker school in his by in Cumberland, when Dalton was just 12 years old he started teaching there. When he was 14, he spent a year working as a farmhand but decided to return to teaching — this time as an assistant at a Quaker boarding school
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Let's review the three basic laws before we get into Dalton's theory.
1. Law of conservation of mass
The law of conservation of mass states that the net change in mass of the reactants and products before and after a chemical reaction is zero. This means mass can neither be created nor destroyed. In other words, the total mass in a chemical reaction remains constant.
This law was formulated by Antoine Lavoisier in It was later found to be slightly inaccurate, as in the course of chemical reactions mass can interconvert with heat and bond energy. However, these losses are very small, several orders of magnitude smaller than the mass of the reactants, so that this law is an excellent approximation.
Does the following chemical reaction obey the law of conservation of mass?
\[\ce{Ca(OH)2 + CO2 -> CaCO3 + H2O}\]
The mass of \(\ce{Ca}\), \(\ce O\), \(\ce H,\) and \(\ce C\) are 40u, 16u, 1u, and 12u, respectively.
Yes, they obey the law of conservation of mass. Let's