How do you write the balanced equation for strontium hydroxide and zirconium (I) perchlorate
1 answer:
The law of conservation of mass states that the mass of a system must remain constant everytime, it can neither be created or destroyed. This means the number of atoms of each element on reactant side must equal the number of atoms of each element on product side.
First we figure out the chemical formula for each compound by taking advantage of oxidation states which are able to tell us whether an element will lose or gain an electron
Strontium hydroxide?
Sr is an alkaline earth metal which has 2 valence electrons that when both are lost it has an oxidation state of +2. Since we know the hydroxide ion has a charge of -1, , Then two
are needed to form compound, hence we have
zirconium (I) perchlorate?
The oxidation state of zirconium is +1 since it is stated that we have zirconium(I). Converserly, perchlorate has a -1 charge which further proves that zirconium has a +1 oxidation state
The product would have a strontium diperchlorate because we know from earlier that Sr has a +2 oxidation state, and we would also have ZrOH because Zr has a +1 oxidation state and has a -1 charge
The unbalanced equation with all chemicals formulas would be
Using the law of conservation of mass, it is clear that there is 1 molecule of on reactant side as compared to 2 molecules of
on product side. On the other hand, the are 2 molecules of
on reactant side and 1 molecule of
on product side. To balance we add a coefficient of 2 on
and a coefficient of 2 on ZrOH,
.
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Answer:
Q = 0.50
No
Left
Explanation:
At a generic reversible equation
aA + bB ⇄ cC + dD
The reaction coefficient (Q) is the ratio of the substances concentrations:
Solids and liquid water are not considered in this calculus.
When the reaction achieves equilibrium (concentrations are constant), the Q value is named as Kc, which is the equilibrium constant of the reaction. If Q > Kc, it indicates that the concentration of the products is higher, so, the reaction must progress to the left and form more reactants; if Q < Kc, than the concentrations of the reactants, are higher, so, the reaction progress to the right.
In this case:
Q =
Q = 0.50
So, Q > Kc, the reaction is not at equilibrium and it progresses to the left.