Equilibrium Expressions

2SO₂(g)+O₂(g)⇌2SO₃(g)
Adding SO₂(g) will

• shift equilibrium right

• shift equilibrium left

• increase rate of reaction

• have no change

Tags

NGSS.HS-PS1-5

For the following reaction: H₂(g) + Cl₂ (g) ↔ 2HCl(g), calculate the concentration of HCl when K_eq= 2.3x10^-5, [H₂]= 0.0056mol, [Cl₂]= 0.0048mol.

• 6.2 x 10^-10 M

• 2.5 x 10^-5 M

• 1.1 M

• 1.2 M

A chemical equilibrium exists when:

• reactants are completely changed to products.

• there are equal amounts of reactants and products.

• the rate at which reactants form products becomes zero.

• the rate at which reactants form products is the same as the rate at which products form reactants

Tags

NGSS.HS-PS1-6

What is [H₂O] if K = 1.2,
[CO₂] = 0.846M, & [CH₄]= 0.0713M?
4CuO_(s)+CH_4(g)↔CO_2(g)+4Cu_(s) +2H₂O_(g)

• 0.101 M

• 0.318 M

• 0.0102 M

• 3.77 M

Tags

NGSS.HS-PS1-5

Consider the following reaction :    
SO_{2 (g)} +  NO_{2 (g)} ↔ SO_{3 (g)} + NO (g)  
had reached a state of equilibrium, was found to contain   0.40 M SO₃ , 0.30 M NO, 0.15 M NO₂ , and 0.20 M SO₂. Calculate the equilibrium constant  for this reaction.

• 4

• 0.42

• 0.25

• 1

Tags

NGSS.HS-PS1-7

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

0.600 moles of NO and 0.750 moles of O₂ are placed in an empty 2.00 L flask. The system is allowed to establish equilibrium. What will be the equilibrium concentration of each species in the flask?

2 NO_(g) + O_2(g) ⇄ 2 NO_2(g)

Kc = 5.00 x 10^-6

use 5% rule (no quadratic equation)

• [NO₂] = 4.1x10^-4, [NO] = 0.300, [O₂] = 0.375

• [NO₂] = 2.05x10^-4, [NO] = 0.600, [O₂] = 0.750

• [NO₂] = 2.05x10^-4, [NO] = 0.300, [O₂] = 0.375

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-5

NGSS.HS-PS1-7

A mixture of 0.10 mol of NO, 0.050 mol of H₂, and 0.10 mol of H₂O is placed into a 1.0-L vessel at 300 K. At equilibrium, [NO] = 0.062 M. Determine the equilibrium concentrations of H₂, N₂, and H₂O, then determine Kc. 2 NO_(g) + 2 H_2(g) ⇄ N_2(g) + 2 H₂O_(g)

• Kc = 650

• Kc = 3.58

• Kc = 0.501

• Kc = 50.

For the equilibrium
2SO₃(g) ↔ 2SO₂(g) + O₂(g)
K_c = 4.08x10^-3 at 1000K
What is K_p?

• 3.45 x 10⁵

• 2.99

• 0.335

• 3.4 x 10^-5

Find the K_c for
2NOBr(g) + Cl₂(g) ↔ 2NO(g) + 2BrCl(g)
 if 
2NOBr(g) ↔ 2NO(g) + Br₂(g)
has a K_c = 0.014
Br2(g) + Cl2(g) ↔ 2BrCl(g)
has a K_c = 7.2

• 0.10

• 10

• 1.0 x 10^-3

• 1.0 x 10^-2