Kc Kp

Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x10⁴.
At a higher temperature, K = 1.8x10^-5. Placing the equilibrium mixture in an ice bath (thus lowering the temperature) will...

• cause [A] to increase
• cause [B] to increase
• gave no effect
• cannot be determined

Tags

NGSS.HS-PS1-5

Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x10⁴.
Addition of chemical B to an equilibrium mixture of the above will...

• cause [A] to increase
• cause [C] to increase
• have no effect
• cannot be determined

Tags

NGSS.HS-PS1-5

Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x10⁴.
If you mixed 5.0 mol B, 0.10 mol C, and 0.0010 mol A in a one-liter container, which direction would the reaction initially proceed?

• shift left
• shift right
• have no effect
• cannot be determined

Tags

NGSS.HS-PS1-5

Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x10⁴.
Raising the pressure by lowering the volume of the container will...

• cause [A] to increase
• cause [B] to increase
• have no effect
• cannot be determined

Tags

NGSS.HS-PS1-6

The value of Kc for this reaction is 1.10 at 25 degrees Celsius.  What is the value of Kp for this reaction?
4CuO(s) + CH₄(g) ↔ CO₂(g) + 4Cu(s) + 2H₂O(g)

• 37.2
• 26.9
• 4.63
• 658

What is the proper K_eq for the following reaction? 
   2 NO_(g)  +  O_2(g) ⇌2 NO_2(g)

• K_eq = [NO₂]² / [NO]²[O₂]
• K_eq =  [NO]²[O₂] / [NO₂]²
• K_eq = [NO]²[O₂][NO₂]²
• K_eq = 2[NO][O₂] / 2[NO₂]

Tags

NGSS.HS-PS1-6

Consider the following reaction:
2SO_2(g) + O_2(g) ⇄ 2SO_3(g) +  197 kJ/mol Which of the following will not shift the equilibrium to the right?

• Adding more O₂
• Adding a catalyst
• increasing the pressure
• Lowering the temperature

Consider the following equilibrium system:
CaCO_3(s) ⇄ CaO_(s) + CO_2(g) 
Which one of the following changes would cause the above system to shift left?

• Add more CaO
• Remove CO₂
• Remove CaCO₃
• Add a catalyst

Use the K_a values to determine whether there are more products or reactants at equilibrium for the given reaction.
K_a NH₄⁺¹= 5.6x10^-10
K_a HCO₃^-1= 4.8x10^-11

• More  products. 
  K_a NH₄⁺¹ > K_a HCO₃^-1
• More  products. 
  K_a NH₄⁺¹ < K_a HCO₃^-1
• More  reactants. 
  K_a NH₄⁺¹ > K_a HCO₃^-1
• More  reactants. 
  K_a NH₄⁺¹ < K_a HCO₃^-1

Identify the incorrect statement about achieving equilibrium.

• achieved when product and reactant concentration is equal
• achieved when forward + reverse rxn rates are same
• achieved when concentration of reactants is constant
• achieved when rxn quotient Q = equilibrium constant

Tags

NGSS.HS-PS1-6