A piece of magnesium metal weighing 1.56 g is placed in 100.0 mL of
Interpretation:
The concentrations of
Concept introduction:
The expression to calculate the electrode potential of cell
Here,
The number of moles of a compound can be calculated as:
The number of moles of a compound can be calculated as:
The relationship between liters and milliliters can be expressed as:
To convert milliliters to liters, the conversion factor is
The relation between equilibrium constant and standard reduction potential of a cell is given as:
Here,
the equilibrium constant is calculated as:
For a general reaction:
The general formula for writing equilibrium expression for the reaction is given as:
Here,
A and B are reactants, C and D are products, and
Answer to Problem 79AP
Solution:
Explanation of Solution
Given information: The mass of magnesium is
Volume of
Concentration of
The mass of
Thus, the conversion factor becomes
Invert the conversion factor and multiply it with
Molarity is the number of moles of solute dissolved in
Multiply the conversion factor with volume to calculate the moles of
Write the balanced chemical equation between
According to the above reaction,
Multiply the conversion factor with the calculated moles of
Calculate the remaining moles of
The mass of
Thus, the conversion factor becomes
Multiply the conversion factor with
According to the above reaction, the mole ratio of
The formula to calculate the standard electrode potential
From the standard reduction potential table, the reduction potential of
From the reaction, it is clear that the reduction of
Substitute
Now, calculate the equilibrium constant as follows:
According to the reaction, the number of electrons transferred is 2.
Substitute 2 for
Let
According to the above, the expression of
Substitute
As the value of
On solving,
So, the concentration of
The concentration of
The value of
As the value of
The concentrations of
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Chapter 19 Solutions
Chemistry
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