CH 18

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This deck includes 14 flashcards for Chemistry. Use it to review key material, focus on weak cards, and prepare for your next exam with StudyLess.

1. 01

   What is chemical equilibrium?

   Rate of forward and reverse reaction are the same; concentrations of reactants and products remain constant.

2. 02

   What is a reversible reaction?

   A reaction in which products can reform the reactants.

3. 03

   What type of reactions are not reversible?

   Reactions that form ionic compounds (ex. Neutralization reaction).

4. 04

   What factor changes the equilibrium constant (K)?

   Temperature.

5. 05

   How is the equilibrium constant expression (K) written for nA + mB ⇌ xC + yD?

   K = ([C]^x * [D]^y) / ([A]^n * [B]^m).

6. 06

   What is the equilibrium constant (K)?

   Ratio between mathematical product of concentration of product and reactants at equilibrium.

7. 07

   Why are concentrations of pure solids or liquids not written in equilibrium expressions?

   Their concentration does not change (only gas & aqueous solutions).

8. 08

   To which state of matter do changes in pressure apply in Le Châtelier's principle?

   Only applies to gases.

9. 09

   What happens when temperature increases in the 2NO2(g) ⇌ N2O4(g) + energy system?

   More of the endothermic reaction occurs, so more brown NO2 forms.

10. 10

    What happens to the equilibrium of A+B ⇌ C+D if the concentration of A is increased?

    Shifts to the right to relieve stress by decreasing the concentration of A.

11. 11

    What happens when energy as heat is taken away from the 2NO2(g) ⇌ N2O4(g) + energy system?

    Exothermic reaction is favored, more N2O4 is produced, and the bottle appears lighter.

12. 12

    What happens to the equilibrium of N2(g) + 3H2(g) ⇌ 2NH3(g) if pressure is increased?

    Equilibrium shifts to the right because there are less moles (less pressure).

13. 13

    What is Le Châtelier's principle?

    If a system at equilibrium is under stress, the equilibrium shifts to relieve the stress.

14. 14

    What happens to the equilibrium of N2(g) + 3H2(g) ⇌ 2NH3(g) + energy if temperature is increased?

    Endothermic reaction is favored, so equilibrium shifts to the left.