Reversible Reactions and Equilibrium Assignment and Quiz

Consider the reaction. N2(g) + 3H2(g) <-> 2NH3(g) At equilibrium, the concentrations of the different species are as follows. [NH3] = 0.105 M [N2] = 1.1 M [H2] = 1.50 M What is the equilibrium constant for the reaction at this temperature?

0.0030

Consider the reaction below. PCl5(G) <-> PCl3 (g) + Cl2(g) At 500 K, the reaction is at equilibrium with the following concentrations. [PCI5]= 0.0095 M [PCI3] = 0.020 [CI2] = 0.020 M What is the equilibrium constant for the given reaction?

0.042

At equilibrium at 1200°C, [I2] = 9.5 ×10-2 M and [I] = 3.2 × 10-2 M. What is the value of Keq for this system? In this system, the equilibrium lies to the _____, and the reaction favors the _______

1.1 × 10-2 left reactants

Carbon monoxide (CO) reacts with hydrogen (H2) to form methane (CH4) and water (H2O). CO(g) + 3H2(g) <-> CH4(g) + H2O(g) The reaction is at equilibrium at 1,000 K. The equilibrium constant of the reaction is 3.90. At equilibrium, the concentrations are as follows. [CO] = 0.30 M [H2] = 0.10 M [H2O] = 0.020 M What is the equilibrium concentration of CH4 expressed in scientific notation?

5.9 x 10-2

The equilibrium constant for this system is 8.5 × 10-3. If the equilibrium concentration of NH3 is 9.2 × 10-2 M, what is the equilibrium concentration of H2S? In this system, the equilibrium lies to the _____, and the reaction favors the _____

9.2 × 10-2 M left reactants

Although I2 is the stable form of iodine at low temperatures, at high temperatures the molecule can dissociate: mc001-1.jpg What is the equilibrium constant expression for this system?

A

Ammonium hydrogen sulfide (NH4HS) can decompose to ammonia and hydrogen sulfide: NH4HS(s) <-> NH3(g) + H2S(g) What is the equilibrium constant expression for this system?

B - Keq = [NH3][H2S]

Identify the correct equilibrium constant expression for this equation: 2NO(g) + O2(g) <-> 2NO2(g)

B - Keq = [NO2]2/[NO]2[O2]

Identify the correct equilibrium constant expression for this equation: C6H12O6(s) + 6O2(g) <-> 6CO2(g) + 6H2O(g)

C - Keq = [CO2]6[H2O]6/[O2]6

Consider the following reversible reaction. 2H2O(g) <-> 2H2(g) + O2(g) What is the equilibrium constant expression for the given system?

D

Which represents the correct equilibrium constant expression for the reaction below? Cu(s) + 2Ag+(aq) <-> Cu2+(aq) + 2Ag(s)

D

Consider the reaction below. 2NH2O5(g) <-> 4NO2(g) + O2(g) If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?

The concentrations of the products and reactants do not change.

Consider the following chemical reaction: 2CH4(g) es002-1.jpg C2H2(g) + 3H2(g) Describe what is happening within the system when it is at equilibrium in terms of concentrations, reactions that occur, and reaction rates.

The equilibrium in the system is a dynamic equilibrium. At equilibrium, the rate of the forward reaction (CH4 decomposing into C2H2 and H2) is equal to the rate of the reverse reaction (C2H2 and H2 reacting to form CH4). At equilibrium, the concentrations of all substances are not changing. At equilibrium, both the forward and reverse reactions are still occurring.

Consider the equilibrium system below. NH4Cl(s) <-> NH4Cl(g) If the system is at dynamic equilibrium, which statement is true?

The rate of sublimation of the NH4CI crystals is equal to the rate of solidification of the NH4CI vapors.

The reaction below is at dynamic equilibrium. N2(g) + 3H2(G) <-> 2NH3(g) Which statement is true for the equilibrium system?

The rate of the forward reaction equals the rate of the reverse reaction.

In the atmosphere, under the effect of ultraviolet rays, oxygen molecules combine to form ozone molecules, and ozone molecules also photodissociate to form oxygen molecules. Which of the following would be observed if this reaction is in dynamic equilibrium?

The rates of the forward and reverse reactions will remain the same.

Which lists all of the substances that appear in equilibrium constant expressions?

pure gas and aqueous solution