Answer:
The equation ![\frac{[HI]^{2} }{[H_{2}[I_{2} ] }](https://tex.z-dn.net/?f=%5Cfrac%7B%5BHI%5D%5E%7B2%7D%20%7D%7B%5BH_%7B2%7D%5BI_%7B2%7D%20%5D%20%20%7D)
represent
(1) law of mass action
(2) mass action expression
(3) equilibrium constant expression
Explanation:
At a given temperature, the rate of a reaction at a particular instant is proportional to the product of the active masses of the reactants at that instant raised to powers which are numerically equal to the numbers of their respective molecules in the stoichiometric equation describe the reaction.
Answer:
The answer is Relative plenitude alludes to the amount of a specific isotope is available in a given measure of test.
Explanation:
The 'relative plenitude' of an isotope implies the level of that specific isotope that happens in nature. Most components are comprised of a blend of isotopes. The total of the rates of the particular isotopes must indicate 100%. The relative nuclear mass is the weighted normal of the isotopic masses. The percent plenitude of every sort of sweets reveals to you what number of every sort of Aufbau there are in each 100 CANDIES. Percent wealth is additionally relative plenitude. This is only a method for giving us a photo on which kind exists all the more every now and again.
Answer
Always have different numbers of electrons, protons, and neutrons.
Explanation:
Every element is unique and has an atomic number. That number tells you the number of protons in every atom of the element. The atomic number is also called the proton number.
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Answer:
The equilibrium will remain at the same conditions because there is no effect and difference in the partial pressure which in turn affect the equilibrium state.
Explanation:
- As Nitrogen is an inert gas therefore it will not react with either the reactants or products.
- Also as the addition is being made by maintaining the volume of flask as constant, thus there will be no difference in the partial pressure of the individual components of the mixture by addition of the Nitrogen gas.
- An increase in pressure is observed but the effect is not aiding or retreating the equilibrium conditions
