Why is it important to ensure that a chemical equation is balanced before calculating the equilibrium constant?

Equilibrium Constant Concepts

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Chemistry
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11th - 12th Grade
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Hard

Patricia Brown
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10 questions
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1.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
To ensure the reaction proceeds
To make the calculation easier
To determine the initial concentrations
To accurately reflect the stoichiometry of the reaction
2.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What does it mean when a reaction reaches equilibrium?
The temperature of the system decreases
The reaction stops completely
The concentrations of reactants and products are equal
The forward and reverse reactions occur at the same rate
3.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
Why do we use Kc instead of Kp in this scenario?
Because the reaction is exothermic
Because the concentrations are given in molarity
Because the substances are solids
Because the reaction is irreversible
4.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
In the equilibrium constant expression, why are products placed on top?
Because the expression is a ratio of products to reactants
To emphasize the importance of products
To ensure the units cancel out
To simplify the calculation
5.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How does the stoichiometry of a reaction affect the equilibrium constant expression?
It affects the temperature dependence
It changes the units of Kc
It has no effect on the expression
It determines the exponents in the expression
6.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
What is the significance of using equilibrium concentrations in the Kc expression?
They simplify the calculation
They are always higher than initial concentrations
They reflect the system at equilibrium
They are easier to measure
7.
MULTIPLE CHOICE QUESTION
30 sec • 1 pt
How is the equilibrium constant Kc calculated from equilibrium concentrations?
By dividing the concentration of products by reactants, each raised to their stoichiometric coefficients
By multiplying the concentrations of reactants
By adding the concentrations of reactants and products
By subtracting the concentration of reactants from products
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