Factors Affecting Equilibrium

Equilibrium for 2CrO₄^2- + 2H⁺ → Cr₂O₇^2- + H₂O. What happen when H⁺ ion are added to the system?

• Position of equilibrium will shift to left
• Color of system will turn from orange to yellow
• K_c will be higher
• Equilibrium will shift to right to decrease the added H⁺ ion

Tags

NGSS.HS-PS1-5

1st statement

Increasing reaction temperature can increase the

yield for all reversible chemical reactions.

2nd statement

Increasing reaction temperature can shorten the

time needed to attain equilibrium for all reversible

chemical reactions.

• Both statements are true and the 2^nd statement is a correct explanation of the 1^st statement

• Both statements are true but the 2^nd statement is NOT a correct

• The 1^st statement is false but the 2^nd statement is true

• Both statements are false

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Refer to the following reversible reaction :

X₂(g) + 3Y₂(g) <=== > XY₃(g)

Which of the following combinations shows the effects of a catalyst on the rate of forward reaction, the rate of backward reaction and the yield of XY₃(g) ?

• Rate of forward reaction

  increased

  Rate of backward reaction

  increased

  Yield of XY₃(g)

  unchanged

• Rate of forward reaction

  unchanged

  Rate of backward reaction

  unchanged

  Yield of XY₃(g)

  unchanged

• Rate of forward reaction

  increased

  Rate of backward reaction

  decreased

  Yield of XY₃(g)

  increased

• Rate of forward reaction

  decreased

  Rate of backward reaction

  increased

  Yield of XY₃(g)

  decreased

Tags

NGSS.HS-PS1-5

The following system attained equilibrium at a certain temperature :

2SO₂(g) + O₂(g) <===> 2SO₃(g)

Which of the following statements is / are correct when the volume of the system is decreased while the temperature remains unchanged ?

(1) The value of K_C increases.

(2) The equilibrium position shifts to the right.

(3) The rate of decomposition of SO₃(g) increases.

• (1) only

• (2) only

• (1) and (3) only

• (2) and (3) only

Tags

NGSS.HS-PS1-5

In a closed container and at a certain temperature, the following equilibrium was attained :

COCl₂(g) <===> CO(g) + Cl₂(g)

Which of the following statements is / are correct ?

(1) CO(g) and Cl₂(g) must be of the same concentration.

(2) The rate of decomposition of COCl₂(g) is equal to the

rate of formation of CO(g).

(3) The equilibrium constant K_c for the reaction increases

when the volume of the container increases.

• (1) only

• (2) only

• (1) and (3) only

• (2) and (3) only

Tags

NGSS.HS-PS1-5