pure sample of ammonia contains 14 g of nitrogen and 3 grams of hydrogen. A second sample of pure ammonia contains 28 g nitrogen and 6 g of hydrogen. This is an example of the:
3 points
law of universal gravitation
law of multiple proportions
law of definite proportions
law of mass action
Answers
Answer:
Hey mate here is your answer
Explanation:
It's contains of Law of multiple proportion.
Option two is the correct answer
Answer:
It is an example of law of multiple proportions.
Explanation:
The statement that the weights of one element that combine with a fixed weight of the other are in a ratio of small whole numbers when two elements combine to form more than one compound is known as the law of multiple proportions. For instance, there are five distinct oxides of nitrogen, and the ratio of oxygen to nitrogen in the form of 14 grams is 8, 16, 24, 32, and 40 grams, or 1, 2, 3, 4, 5. John Dalton, an English chemist, announced the law in 1803, and its application to a wide variety of compounds served as the strongest argument in support of Dalton's theory that matter is made up of atoms that cannot be divided.
Take into account the elements oxygen and carbon. They combine in one way to form carbon dioxide, a well-known compound. There are 32.0 grams of oxygen for every 12.0 grams of carbon in each carbon dioxide sample. This simplifies to a mass ratio of 2.66 to 1 for oxygen and carbon by dividing 32.0 by 12.0. Carbon monoxide is an additional compound that results from the combination of carbon and oxygen. For every 12.0 grams of carbon in a sample of carbon monoxide, there are 16.0 grams of oxygen. The mass ratio of carbon to oxygen is 1.33 to 1.There is exactly twice as much oxygen in carbon dioxide as there is in carbon monoxide. The law of multiple proportions is demonstrated by this illustration: Small whole numbers are used to represent the ratio of the distinct masses of the two elements when they combine to form more than one compound when the same two elements are present.
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