Consider the following reversible reaction. 2H2O(g)<—>2H2(g)+O2(g) What is the equilibrium constant expression for the giv
2 answers:
Answer : The equilibrium constant expression will be,
Explanation :
The given balanced chemical reaction is,
The equilibrium expression for the reaction is determined by multiplying the concentrations of products and divided by the concentrations of the reactants and each concentration is raised to the power that is equal to the coefficient in the balanced reaction.
The concentrations of pure solids are constant that is they do not change. Thus, they are not included in the equilibrium expression.
So, the equilibrium constant expression will be,
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Answer:
Approximately .
Explanation:
The gallium here is likely to be produced from a solution using electrolysis. However, the problem did not provide a chemical equation for that process. How many electrons will it take to produce one mole of gallium?
Note the Roman Numeral "" next to
. This numeral indicates that the oxidation state of the gallium in this solution is equal to
. In other words, each gallium atom is three electrons short from being neutral. It would take three electrons to reduce one of these atoms to its neutral, metallic state in the form of
.
As a result, it would take three moles of electrons to deposit one mole of gallium atoms from this gallium solution.
How many electrons are supplied? Start by finding the charge on all the electrons in the unit coulomb. Make sure all values are in their standard units.
.
.
Calculate the number of electrons in moles using the Faraday's constant. This constant gives the size of the charge (in coulombs) on each mole of electrons.
.
It takes three moles of electrons to deposit one mole of gallium atoms . As a result,
of electrons would deposit
of gallium atoms
.