Equilibrium constant

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

If the equilibrium constant is much greater than one (K >> 1) then

• Equilibrium is not established.
• Equilibrium lies to the right (products are favored)
• Equilibrium lies to the left (reactants are favored)
• Neither products or reactants are favored.

Tags

NGSS.HS-PS1-6

If the equilibrium constant is much less than one (K << 1) then

• Equilibrium is not established.
• Equilibrium lies to the right (products are favored)
• Equilibrium lies to the left (reactants are favored)
• Neither products or reactants are favored.

Tags

NGSS.HS-PS1-6

N₂O₄(g) ↔ 2 NO₂(g)
What is the concentration equilibrium constant expression?

• K_c = [NO₂]²/[N₂O₄]
• K_c = [N₂O₄]/[NO₂]²
• K_c = [N₂O₄]²/[NO₂]
• K_c = [NO₂]/[N₂O₄]²

Tags

NGSS.HS-PS1-6

What is the equilibrium-constant expression for 
CO₂(g) + H₂(g) ↔ CO(g) + H₂O(l)

• K_c= [CO][H₂O] / [CO₂][H₂]  
• K_c= [CO₂][H₂] / [CO]
• K_c= [CO₂][H₂] / [CO][H₂O]
• K_c= [CO] / [CO₂][H₂]  

Tags

NGSS.HS-PS1-6

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

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

 SO3(g) +  H2O(g)    ⇄   H2SO4(g)         
At equilibrium [SO3] = 0.400M, [H2O] = 0.480M, [H2SO4] = 0.600M            
 Calculate the value of the equilibrium constant.

• 0.682

• 0.425

• 1.69

• 3.13

• 1.32 x $10^{-2}$  

2SO₂ (g) + O₂ (g) ⇄ 2SO₃ (g)

0.600 M of SO₂ and 0.600M of O₂ are present in a at equilibrium If the Keq = 680, calculate the SO₃ concentration

• 146.88

• 24.23

• 12.12

• 21573

Consider the following equilibrium:

2NO_{2(g) <->} N₂O_4(g)

A 1.00 L flask contains 0.030 mol NO₂ and 0.040 mol N₂O₄ at equilibrium.

The value of K_eq is

• 0.023

• 0.67

• 1.3

• 44

Tags

NGSS.HS-PS1-6

the reaction A + B  $\leftrightarrow$  E   consists of two steps
step 1   A + B  $\leftrightarrow$  C    (Keq = 1.35)
step 2   C + B  $\leftrightarrow$  E    (Keq = 12.6)

What would the Keq be for the net equation below

E  $\leftrightarrow$  A + B

• 17.01

• 13.95

• 9,33

• 0.059