Question

As early as 400 B.C., Greek philosophers proposed that matter was made up of particles. During the 1800s, John Dalton linked the idea of atoms with the chemical identity of an element. His atomic theory of matter involved the following postulates. 1. Each element is composed of extremely small particles called atoms. 2. All atoms of a given element are identical to one another in mass and other properties, but the atoms of one element are different from the atoms of other elements. 3. Atoms of an element are not changed into atoms of a different element by chemical reactions: atoms are neither created nor destroyed in chemical reactions. 4. Compounds are formed when atoms of more than one element combine, a given compound always has the same relative number and kind of atoms. Scientists later discovered isotopes, which showed that the second postulate was not entirely true, and nuclear reactions, which showed that the third postulate was not true. Which of the following reactions is possible according to Dalton's atomic theory? N_2 rightarrow O_2 N_2 + O_2 rightarrow 2NO CO_2 rightarrow NO_2 H_2O rightarrow H_2S The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction. This can be gleaned from the third postulate in Dalton's series. Magnesium oxide decomposes into magnesium and oxygen. If 4.03 g of magnesium oxide decomposes to form 2.43 g of magnesium, what mass of oxygen gas is also released in the reaction? Express your answer with the appropriate units.

Answer 1