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

At what time did the reaction establish equilibrium?

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g). Adding O₂ will...

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g). Which change will increase the amount of N₂ at equilibrium?

Consider the reversible reaction:

CO (g) + 2H₂ (g) ⇌ CH₃OH (g) + energy. Cooling the reaction mixture will ___.

Consider the reversible reaction:

CO (g) + 2H₂ (g) ⇌ CH₃OH (g) + energy. Adding a catalyst will____.

What states of matter are omitted when writing K_eq expressions?

2 NO_(g) + O_2(g) ⇌ 2 NO_2(g)

What is the correct expression for equilibrium constant for the chemical reaction above?

Given the equation representing a reaction:

N₂O_4(g) ⇌ 2NO_2(g)

Which statement describes this reaction at equilibrium?

Consider the following reaction. What would be the equilibrium constant expression?

4Br₂(g) + CH₄(g) ⇌ 4HBr(g) + CBr₄(g)

Calculate [H₂O] if K_eq = 1.2,

[CO₂] = 0.846M, and [CH₄]= 0.0713M

4CuO_(s) +CH_4(g) ⇌ CO_2(g)+4Cu_(s) +2H₂O_(g)

At elevated temperatures ammonium carbonate, NH₂COONH₄, is in equilibrium with NH₃ and CO₂ according to the equation

NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g)

What is the equilibrium expression for this reaction?

Consider the reversible reaction

N₂ (g) + O₂ (g) + 181 kJ ⇌ 2NO (g).

If N₂ is removed...

The following reaction :

SO_{2 (g)} + NO_{2 (g)} ⇌ SO_{3 (g)} + NO (g)

established equilibrium and 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.

When K_eq < 1,

Select all of the statements that are always correct about dynamic equilibrium

The statement that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:

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.

An equilibrium constant with a large value, e.g. K_eq = 1000, indicates ___.

What is the K_eq expression for this reaction?

2 NO_(g) + O_2(g) ⇌ 2 NO_2(g)

Which of the following is an example of a change that does NOT affect the equilibrium position?

Increasing the concentration of the reactants will ___.

If the volume of the container is decreased at constant temperature, this will ____.

2NO_{2 (g)} ⇌ N₂O_{4 (g)}

For the reaction...

SO₂ + O₂ ⇌ SO₃

If the concentration of SO₂ is increased, the system will ___

For the reaction...

heat + N₂ + O₂ ⇌ 2NO

If O₂ is removed, the concentration of N₂ will _______.

For the reaction...

heat + N₂ + O₂ ⇌ 2NO

If NO is removed from the system, the concentration of N₂ will _______.

For the reaction...

H_{2 (g)} + Cl_{2 (g)} ⇌ 2HCl _(g) + heat

If the pressure in the system is increased, the system will _______.

For the reaction...

N_{2 (g)} + 3 H_2(g) ⇌ 2 NH_{3 (g)}

If the pressure in the system is decreased, which substance will increase in concentration?

For the reaction at equilibrium:

4H₂(g) + CS₂(g) ⇌ CH₄(g) + 2H₂S(g)

If some CH₄ is removed, what will happen to the concentration of H₂S in order to re-establish equilibrium?

For a chemical system at equilibrium, the concentrations of both the reactants and the products must

Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:

H₂(g) + I₂(g) + energy ⇌ 2HI(g)

When the concentration of H₂(g) is increased by adding more hydrogen gas to the container at constant temperature, the system responds by

A precipitation reaction establishes equilibrium:

BaCl₂(aq) + Na₂SO₄(aq) ⇌ 2 NaCl(aq) + BaSO₄(s)

If more BaSO₄(s) is added to the equilibrium system, how will the system respond?

A saturated solution of silver sulfate is prepared in water, and the following equilibrium is established:

Ag₂SO₄(s) ⇌ 2 Ag⁺(aq) + SO₄^2-(aq)

If a sample of silver nitrate is added to the solution, the mass of the solid silver sulfate will ____.

Consider the reaction at equilibrium:

heat + A₂(g) + 3 B₂(g) ⇌ 2 AB₃(g)

Which of the following stresses would cause a shift to the right?

(Select all that apply)

For the reaction:

4H₂(g) + CS₂(g) ⇌ CH₄(g) + 2H₂S(g);

If the container volume is decreased at constant temperature, the moles of H₂S present in the container will ___

For the reaction

N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + 92 kJ

What happens to the equilibrium position when a catalyst is added to this reaction?

2SO₂(g)+O₂(g)⇌2SO₃(g)

Adding SO₃(g) at constant temperature will ___.

Consider the reaction at equilibrium:

heat + A₂(g) + 3 B₂(g) ⇌ 2 AB₃(g)

The value of the equilibrium constant will be changed by

An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will

For the reaction...

SO_2(g) + O_2(g) ⇌ SO_3(g)

If the concentration of SO_2(g) is increased, the system will ___________ to re-establish equilibrium.

For the reaction...

SO_2(g) + O_2(g) ⇌ SO_3(g)

If the equilibrium shifts to the right, the concentration of O_2(g) will ___________.

For the reaction...

energy + N_2(g) + O_2(g) ⇌ 2NO_(g)

If O_2(g) is removed, the concentration of N₂ will _______.

For the reaction at equilibrium

heat + N_2(g) + O_2(g) ⇌ 2NO_(g)

If the temperature of the system is lowered, the system will:

For the reaction at equilibrium:

N_{2 (g)} + 3 H_2(g) ⇌ 2 NH_{3 (g)}

If the pressure in the system is increased, the reaction will __________________.

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...

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...

A_(g) + B_(aq) ⇌ C_(s)

ΔH_rxn= -453 kJ/mol

If [B] is decreased, then the reaction will _______.

2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

Removing O₂(g) will

A_(g) + B_(aq) ⇌ C_(g) + D_(g)

ΔH_rxn= 240 kJ/mol

If the volume of the reaction container increases at constant temperature, the system will ____.

A_(g) + B_(aq) ⇌ C_(s)

ΔH_rxn= -453 kJ/mol

If additional solid C is added to the container, then the reaction will _______.

2SO₂(g)+O₂(g) ⇌ 2SO₃(g) is an exothermic reaction.

An increase in temperature will...

For the equilibrium reaction 2NH₃(g) + 22 kJ ⇌ N₂(g) + 3H₂(g), which of the following changes would result in the formation of more N₂ and H₂ at equilibrium?

Increasing the pressure on the reaction: 2NO_{2 (g)} ⇌ N₂O_{4 (g)} will:

For the reaction: 4H₂(g) + CS₂(g) ⇌ CH₄(g) + 2H₂S(g);

If we remove some CH₄ after equilibrium has been reached, what will happen to the partial pressure exerted by H₂S?

For the reaction: 4H₂(g) + CS₂(g) ⇌ CH₄(g) + 2H₂S(g);

If we decrease the volume of the container this takes place in what will happen to the concentration of H₂S?

For the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + 92 kJ;

what happens to the equilibrium position by adding a catalyst to this reaction?

The following reaction establishes equilibrium:

PCl₅(g)  ⇌ PCl₃(g) + Cl₂(g)

Which of the following graphs correctly shows how the system will change to re-establish equilibrium if additional Cl₂(g) is added at 20 seconds?

If the reaction quotient Q has a smaller value than the related equilibrium constant, K, _________

If the reaction quotient Q has a value larger than the related equilibrium constant, K _________

Consider the following reaction :    

SO_{2 (g)} +  NO_{2 (g)} ⇌ SO_{3 (g)} + NO (g)  

After achieving equilibrium, the system was found to contain  

0.40 mol L^-1 SO₃ ,  0.30 mol L^-1 NO, 0.15 mol L^-1 NO₂ , and 0.20 mol L^-1 SO₂.

Calculate the equilibrium constant for this reaction. 

What is the equilibrium constant expression (K_c) for:

Fe₃O₄(s) + 4H₂(g) ⇌ 3Fe(s) + 4H₂O(g)

How is the reaction quotient used to determine whether a system is at equilibrium?

The value of the equilibrium constant, K_p for the reaction below is 3.1 × 10^-4 at 700K.

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Given the initial partial pressure of the gases, P_N2 = 0.411 atm; P_H2 = 0.903 atm; P_NH3 = 0.224 atm, calculate the value of the reaction quotient, Q.

The value of the equilibrium constant, K_p for the reaction below is 3.1 × 10^-4 at 700K.

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Given the initial partial pressure of the gases, P_N2 = 0.411 atm; P_H2 = 0.903 atm; P_NH3 = 0.224 atm. Predict the direction in which the reaction will proceed at 700 K.

For the reaction system:

2HI (g) ⇌ H₂ (g) + I₂ (g)

K_c = 0.020 at 720 K

If the initial concentrations of HI, H₂ and I₂ are all 1.50 × 10^-3 M at 720 K, which one of the following statements is correct?

For the reaction, N₂O₄ (g) ⇌ 2NO₂ (g), K_c = 0.21 at 100^oC. At initial, the [N₂O₄] = 0.12 M and [NO₂] = 0.55 M. Is the reaction at equilibrium? If not, in which direction it is progressing?

For the reaction at equilibrium:

H_{2 (g)}  + Cl_{2 (g)} ⇌  2HCl _(g)  +  heat

If the temperature is lowered, the system will

What is the effect of increasing the pressure on the following equilibrium?

2NO(g) + O₂ (g) ⇌2NO₂(g)

At elevated temperatures ammonium carbonate, NH₂COONH₄, is in equilibrium with NH₃ and CO₂ according to the equation;

NH₂COONH₄(s) ⇌ 2 NH₃(g) + CO₂(g)

What is the equilibrium expression for this reaction?

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.

Find the K_c for 2NOBr(g) + Cl₂(g) ⇌ 2NO(g) + 2BrCl(g)

 if  2NOBr(g) ⇌ 2NO(g) + Br₂(g) K_c = 0.014

and

Br₂(g) + Cl₂(g) ⇌ 2BrCl(g) K_c = 7.2

The value of the equilibrium constant, K_p for the reaction below is 3.1 × 10^-4 at 700K.

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Given the initial partial pressures of the gases, P_N2 = 0.5 atm; P_H2 = 0.1 atm; P_NH3 = 0.2 atm.

How will the system proceed to establish equilibrium?

For the reaction at equilibrium:

H_{2 (g)}  + Cl_{2 (g)} ⇌  2HCl _(g)  +  heat

If the temperature is increased, the value of the equilibrium constant will

Nitrosyl bromide decomposes according to the following equation:

2 NOBr(g) ⇌ 2NO(g) + Br₂(g)

A 0.64 mol sample of NOBr was placed in an evacuated 1.00 L flask. At equilibrium, the flask contained 0.46 mol of NOBr. How many moles of NO and Br₂ are in the flask at equilibrium?

For the reaction at equilibrium:

H_{2 (g)}  + Cl_{2 (g)} ⇌  2HCl _(g)  +  heat

If the temperature is increased,

Carbon monoxide can react with fluorine gas as shown in the equation:

CO(g) + F₂(g) ⇌ COF₂(g)

A container is filled with COF₂ and the system is allowed to achieve equilibrium. After 15 minutes, some F₂ gas is removed from the container. Which of the following graphs shows how the system will respond to establish a new equilibrium?

If the reaction quotient Q has a smaller value than the related equilibrium constant, K, _________

If the reaction quotient Q has a value larger than the related equilibrium constant, K _________

The value of the equilibrium constant, K_p for the reaction below is 3.1 × 10^-4 at 700K.

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Given the initial partial pressure of the gases, P_N2 = 0.411 atm; P_H2 = 0.903 atm; P_NH3 = 0.224 atm, calculate the value of the reaction quotient, Q.

The value of the equilibrium constant, K_p for the reaction below is 3.1 × 10^-4 at 700K.

N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)

Given the initial partial pressure of the gases, P_N2 = 0.411 atm; P_H2 = 0.903 atm; P_NH3 = 0.224 atm. Predict the direction in which the reaction will proceed at 700 K.

For the reaction system:

2HI (g) ⇌ H₂ (g) + I₂ (g)

K_c = 0.020 at 720 K

If the initial concentrations of HI, H₂ and I₂ are all 1.50 × 10^-3 M at 720 K, which one of the following statements is correct?

For the reaction, N₂O₄ (g) ⇌ 2NO₂ (g), K_c = 0.21 at 100^oC. At initial, the [N₂O₄] = 0.12 M and [NO₂] = 0.55 M. Is the reaction at equilibrium? If not, in which direction will the reaction proceed?