The coefficient for aluminium is 4.
Explanation:
We have the following chemical reaction:
Al + O₂ → Al₂O₃
In order to balance the chemical equation the number of the atoms entering the reaction should be equal to the number of atoms leaving the reaction.
2 Al + 3/2 O₂ → Al₂O₃
However we need integer numbers so we multiply everything with 2.
4 Al + 3 O₂ → 2 Al₂O₃
The coefficient for aluminium is 4.
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Answer:
e. 327/227
Explanation:
This is the correct standard pressure.
Answer:
[H2] = [I2] = 0.64M; [HI] = 4.72M
Explanation:
Based on the reaction:
H2 + I2 ⇄ 2HI
The K is defined as:
k = 54.3 = [HI]² / [H2] [I2]
<em>Where [] is molar concentration of each reactant at equilibrium</em>
As the initial concentration of HI is 6mol/dm^3 = 6M the equilibrium concentration of each reactant is:
[H2] = X
[I2] = X
[HI] = 6 - 2X
<em>Where X is reaction coordinate</em>
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Replacing:
54.3 = [6-2X]² / [X] [X]
54.3X² = 4X² - 24X + 36
0 = -50.3X² - 24X + 36
Solving for X:
X = -1.12. False solution, produce negative concentrations
X = 0.64M. Right solution
Replacing:
[H2] = 0.64M
[I2] = 0.64M
[HI] = 6 - 2*0.64M = 4.72M
Equilibrium concentrations are:
<h3>[H2] = [I2] = 0.64M; [HI] = 4.72M</h3>
Answer:
The equilibrium will go right, increasing the quantities of Y(g) and Z(s), when the amount of X(g) increases.
Explanation:
Equilibrium is a state in which the velocity of the formation of the products is equal to the velocity of the formation of the reactants. Thus, the concentrations remain constant.
By Le Chatêlier's principle, when the equilibrium is disturbed, the equilibrium must shift to reestablish the equilibrium. Thus, when X is put in the container, it intends to decompose and form Y and Z, thus, as higher is the initial X, as higher is the Y and Z formed.