Nuclear reactions involves

1 answer:

6 0

Nuclear reaction involves two reacting particles a heavy target nucleus and a light bombarding particle and produces two new particles a heavier product nucleus and a lighter ejected particle.

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How would you describe the solid-state in terms of motion (ability to move in the space and speed) and distance between molecule

horrorfan [7]

In the gaseous state, the molecules are completely free because there is no intermolecular interaction between the molecules hence they translate at incredibly high velocity.

According to the kinetic theory of matter, the molecules that compose matter are in constant random motion. The nature of this motion varies in the three states of matter which are;

Solid
Liquid and
Gas

In the solid state, the molecules do not translate, they only vibrate and rotate about their mean positions. In the liquids state, the molecules translate but they still have restricted degrees of freedom due to intermolecular interactions. In the gaseous state, the molecules are completely free because there is no intermolecular interaction between the molecules hence they translate at incredibly high velocity.

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An atom of boron has an atomic number of 5 and an atomic mass of 11. The atom contains:. . A. 5 protons, 6 electrons, and 5 neut

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<span>C. 5 protons, 5 electrons, and 6 neutrons</span>

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How many grams of Ag2S2O3 form

Art [367]

Taking into account the reaction stoichiometry, 109.09 grams of Ag₂S₂O₃ are formed when 125 g AgBr reacts completely.

<h3>Reaction stoichiometry</h3>

In first place, the balanced reaction is:

2 AgBr + Na₂S₂O₃ → Ag₂S₂O₃ + 2 NaBr

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

AgBr: 2 moles
Na₂S₂O₃: 1 mole
Ag₂S₂O₃: 1 mole
NaBr: 2 moles

The molar mass of the compounds is:

AgBr: 187.77 g/mole
Na₂S₂O₃: 158 g/mole
Ag₂S₂O₃: 327.74 g/mole
NaBr: 102.9 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

AgBr: 2 moles ×187.77 g/mole= 375.54 grams
Na₂S₂O₃: 1 mole ×158 g/mole= 158 grams
Ag₂S₂O₃: 1 mole ×327.74 g/mole= 327.74 grams
NaBr: 2 moles ×102.9 g/mole= 205.8 grams

<h3>Mass of Ag₂S₂O₃ formed</h3>

The following rule of three can be applied: if by reaction stoichiometry 375.54 grams of AgBr form 327.74 grams of Ag₂S₂O₃, 125 grams of AgBr form how much mass of Ag₂S₂O₃?

$mass of Ag_{2} S_{2} O_{3} =\frac{125 grams of AgBrx327.74 grams of Ag_{2} S_{2} O_{3}}{375.54 grams of AgBr}$