Answer:
It is indeed False
Answer:
27.9 g
Explanation:
CsF + XeF₆ → CsXeF₇
First we convert 73.1 g of cesium xenon heptafluoride (CsXeF₇) into moles, using its molar mass:
As 1 mol of cesium fluoride (CsF) produces 1 mol of CsXeF₇, in order to produce 0.184 moles of CsXeF₇ we would need 0.184 moles of CsF.
Now we convert 0.184 moles of CsF to moles, using the molar mass of CsF:
The model most likely represents a reaction which
Select one:
a. takes place when atoms combine
b. takes place when atoms become inactive
c. does not produce energy in the sun
d. does not produce energy in nuclear power plants
Answer: b: takes place when atoms become inactive
Explanation: the model described above is a nuclear fission reaction, a reasonably controlled reaction that releases energy and is employed in nuclear power plants. In these reactions one Atom is split into two lighter ones and there's a resultant release of energy in the process. The original Atom becomes depleted (inactive) as is the case with Uranium 235.
This reaction is opposed to fusion reactions that occur in nature e.g. the sun, and are basically uncontrollable — involving the combination of two atoms into one.
The chemical equilibrium can take place in a close system and can not be affected by catalyst and is a reversible reaction.
The term "chemical equilibrium" describes a situation in which a chemical reaction's forward reaction rate and reverse reaction rate are equal. In other words, throughout time, the reactant and product concentrations in the reaction mixture do not change. Even if the individual reactions may still be in progress, there is no net change in the reactant or product concentrations at the point of chemical equilibrium. This occurs as a result of the equalisation of the rates at which molecules react to create products and molecules disintegrate into reactants. Even though the reaction is still taking place at the molecular level, the system is in equilibrium and it appears to have stopped.
To know more about chemical equilibrium, here:
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The NH3 sample that will fill and take the shape of a 100.0-milliliter container is NH3(g). Gases such as NH3(g) expand to fill their container, as explained by the ideal gas law and Avogadro's law.
To answer your question about NH3, we need to consider each of the states of matter. Hence, the answer is (3) NH3(g). This is because of the properties that gases have, including the ability to fully expand and take the shape of their container regardless of the volume of the container.
Specifically, any gaseous substance, such as NH3(g), expands to fill its container due to the kinetic energy of the gas molecules and their relatively far-apart spacing compared to solids and liquids. Even a small amount of gas can completely fill even a relatively large container. This phenomenon is due to one of the main gas laws, the ideal gas law, and the properties of gases as stipulated by Avogadro's law that equal volumes of gaseous N₂, H₂, and NH3, at the same temperature and pressure, contain the same number of molecules.
This concept is fundamental in the stoichiometry of gaseous substances and Dalton's law of partial pressures, which states that the total pressure exerted by a mixture of gases is equal to the sum of the pressures that each would exert if it were present alone and occupied the same volume.
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