What is the equilibrium-constant expression for CO 2 (g) + H 2 (g) ↔ CO(g) + H 2 O(l)

K c = [CO][H 2 O] / [CO 2 ][H 2 ]

K c = [CO 2 ][H 2 ] / [CO][H 2 O]

What is the equilibrium expression for: Fe 3 O 4 ( s ) + 4H 2 (g) <=> 3Fe( s ) + 4H 2 O(g) K c =

[Fe] 3 [H 2 O] 4 / [Fe 3 O 4 ] [H 2 ] 4

[Fe 3 O 4 ] [H 2 ] 4 / [Fe] 3 [H 2 O] 4

[Fe] [H 2 O] / [Fe 3 O 4 ] [H 2 ]

Rate of chemical reaction means

concentration of reacting particles

combining reactants with products

Increase in temperature of the reactants can do one of the following

increase collision between the particles thus increasing the rate.

Allow less effective collision between the particles

The rate of reaction normally __________

increases as reactant concentration increases

increases a pressure is increased

decreases with the use of a catalyst

decreases as temperature increases

Curve X on the graph below shows the volume of oxygen formed during the catalytic decomposition of a solution of hydrogen peroxide. Which change would produce the curve Y ?

Adding some 0.1 mol L -1 hydrogen peroxide solution

What is the best definition of rate of reaction ?

The increase in concentration of a product per unit time

The time it takes to use up all the reactants

The rate at which all the reactants are used up

The time it takes for one of the reactants to be used up

Curve X on the graph below shows the volume of oxygen formed during the catalytic decomposition of a solution of hydrogen peroxide. Which change would produce the curve Y ?

Adding some 0.1 mol L -1 hydrogen peroxide solution

Hydrochloric acid is reacted with large pieces of calcium carbonate, the reaction is then repeated using calcium carbonate powder. How does this change affect the activation energy and the collision frequency?

E a stays constant; collision frequency increases

E a increases; collision frequency increases

E a increases; collision frequency stays constant

E a stays constant; collision frequency stays constant

What is K c for the following reaction? 2 NO(g) + O 2 (g) ⇌ 2 NO 2 (g)

K c = [NO 2 ] 2 / [NO] 2 [O 2 ]

K c = [NO] 2 [O 2 ] / [NO 2 ] 2

Given the equation representing a reaction: N 2 O 4 (g) ⇌ 2NO 2 (g) Which statement describes this reaction at equilibrium?

The concentration of N 2 O 4 (g) and the concentration of NO 2 (g) must be constant (but not the same as each other)

The concentration of N 2 O 4 (g) must equal the concentration of NO 2 (g).

The rate of the forward reaction is greater than the rate of the reverse reaction.

The rate of the reverse reaction is greater than the rate of the forward reaction.

The following is true for dynamic equilibrium EXCEPT

Concentration of reactant and product are the same at equilibrium

Both forward and reverse reaction continue at equilibrium

The following statement is true for reaction at dynamic equilibrium EXCEPT

Reaction stop once equlibrium is reached

Reverse and forward rate are the same.

Concentration of reactants and products remain unchanged

Concentration of reactants decreases over time

Equilibrum constant K c for the reaction can be written as

K c = [SO 3 ] 2 /[SO 2 ] 2 [O 2 ] 1

K c = [SO 2 ] 2 [O 2 ] 1 /[SO 3 ] 2

Equilibrium Constant Practice

Quiz

•

10th - 12th Grade

•

Practice Problem

•

Medium

Ghazwa Aldoori

Used 93+ times

FREE Resource

40 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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.

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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.

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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]

5.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

This symbol indicates that a reaction is ____________

reversible

irreversible

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

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

7.

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the activation energy?

the quantity of heat absorbed in a reaction

the minimum energy needed to begin a reaction

the energy given off after reactants collide.

both the energy and frequeny of collisions in increased
the energy difference between reactants and products

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Equilibrium Constant Practice

40 questions

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

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

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

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

This symbol indicates that a reaction is ____________

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

What is the activation energy?

What are [A] and [B]?

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 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,
0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.
Calculate the equilibrium constant for this reaction.

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <=> 3Fe(s) + 4H₂O(g)
K_c =

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Equilibrium Constant Practice

40 questions

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

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

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

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

This symbol indicates that a reaction is ____________

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

What is the activation energy?

What are [A] and [B]?

The following reaction : SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g) had reached a state of equilibrium, was found to contain 0.40 mol L-1 SO3 , and 0.30 mol L-1 NO, 0.15 mol L-1NO2 , and 0.20 mol L-1 SO2. Calculate the equilibrium constant for this reaction.

What is the equilibrium expression for: Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)Kc =

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

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

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 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,
0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.
Calculate the equilibrium constant for this reaction.

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <=> 3Fe(s) + 4H₂O(g)
K_c =