Chemical Equilibrium

What is the effect of increasing the concentration of reactants on the position of equilibrium?

• The equilibrium position shifts towards the reactants
• The equilibrium position is unpredictable
• The equilibrium position shifts towards the products
• The equilibrium position remains unchanged

Tags

NGSS.HS-PS1-5

What is the effect of adding an inert gas to a gaseous reaction mixture at constant volume?

• The equilibrium position is unpredictable
• The equilibrium position remains unchanged
• The equilibrium position shifts towards the side with more moles of gas
• The equilibrium position shifts towards the side with fewer moles of gas

What is the effect of adding a catalyst on the position of equilibrium? 🥽

• The equilibrium position remains unchanged
• The equilibrium position is unpredictable
• The equilibrium position shifts towards the reactants
• The equilibrium position shifts towards the products

What is the effect of increasing the pressure on the position of equilibrium for a gaseous reaction?

• The equilibrium position shifts towards the side with fewer moles of gas
• The equilibrium position remains unchanged
• The equilibrium position shifts towards the side with more moles of gas
• The equilibrium position is unpredictable

What are the two factors to look for when determining if the reaction is at equilibrium?

• Forward reaction rate is faster than the reverse and concentrations are equal
• Forward and reverse reaction rates are equal and concentration is conctant
• Forward and revers reaction rates are equal and concentration is equal
• Forward reaction rate is faster than the reverse and concentration is equal

Tags

NGSS.HS-PS1-6

Identify the incorrect statement about achieving equilibrium.

• achieved when product and reactant concentrations are equal

• achieved when forward and reverse reaction rates are same

• achieved when concentration of reactants is stable/constant

• achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

Tags

NGSS.HS-PS1-5

Which of the two graphs reaches equilibrium?

• The left one.
• The right one.
• Both of them.
• Neither.

Tags

NGSS.HS-PS1-6

At elevated temperatures ammonium carbonate, NH₂COONH₄, is in equilibrium with NH₃ and CO₂ according to the equation;

NH₂COONH₄(s) ↔ 2 NH₃(g) + CO₂(g)

What is the equilibrium expression for this reaction?

• K = 2 [NH₃][CO₂]

  [NH₂COONH₄]

• K = [NH₃]²[CO₂]

  [NH₂COONH₄]

• K = 2 [NH₃][CO₂]

• K = [NH₃]²[CO₂]

Tags

NGSS.HS-PS1-7

When 0.40 mole of SO₂ and 0.60 mole of O₂ are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO_{2 (g)} + O_{2 (g)} ↔ 2SO_{3 (g)}

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO₃. Based on these results, the equilibrium constant, Kc, for the reaction is

• 20

• 10

• 6.7

• 2.0

H_2(g) +I_2(g) ↔ 2HI_(g)

All gases begin with an initial concentration of 2.0 M. Equilibrium is established, and the concentration of HI is known to be 4.8 M. What is the value of the equilibrium constant?

• 1.2

• 2.4

• 32

• 64