Understanding Chemical Equilibrium

What is the main idea behind chemical equilibrium?

• Reactions only occur under high pressure.

• Reactions stop once products are formed.

• Reactions can go both forward and backward.

• Reactions only move forward.

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NGSS.HS-PS1-6

How can the position of equilibrium be altered?

• By adding more light to the reaction.

• By increasing the size of the container.

• By altering concentration, temperature, and pressure.

• By changing the color of the reactants.

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NGSS.HS-PS1-6

What does the equilibrium constant (Keq) represent?

• The speed of the reaction.

• The temperature at which the reaction occurs.

• The molar ratio of products to reactants at equilibrium.

• The color change of the reaction.

In the equilibrium constant expression, what role do the coefficients play?

• They are ignored in the calculation.

• They are added to the concentrations.

• They are used as exponents for the concentrations.

• They are subtracted from the concentrations.

What happens to the equilibrium constant if the temperature changes?

• It remains the same.

• It changes because equilibrium is temperature-dependent.

• It doubles.

• It becomes zero.

Tags

NGSS.HS-PS1-6

What is a RICE table used for?

• To cook rice.

• To calculate equilibrium conditions.

• To measure temperature changes.

• To determine the color of a solution.

Tags

NGSS.HS-PS1-6

In a RICE table, what does the 'C' line represent?

• The initial concentrations.

• The change in concentrations during the reaction.

• The final concentrations.

• The color of the reactants.

What is the initial concentration of HF in the example calculation?

• 3 molar

• 1 molar

• 2 molar

• 0 molar

Tags

NGSS.HS-PS1-5

What type of equation often results from equilibrium calculations?

• Linear equation

• Quadratic equation

• Cubic equation

• Exponential equation

Tags

NGSS.HS-PS1-6

How do you determine the correct solution from a quadratic equation in equilibrium calculations?

• Choose the larger value.

• Consider the initial concentrations to find a feasible solution.

• Use the average of the two solutions.

• Choose the smaller value.