Chemical Equilibrium Concepts

In the ICE table method for solving equilibrium problems, which step involves using the balanced chemical equation to express the equilibrium constant $K$?

According to Le Châtelier's Principle, how will a system at equilibrium respond to the removal of a product?

For the reversible reaction $N_2(g) + 3H_2(g) ightleftharpoons 2NH_3(g)$, how does decreasing the volume of the container affect the equilibrium?

For an exothermic reaction at equilibrium, what is the effect of increasing the temperature?

Why does adding a catalyst to a reaction at equilibrium not change the equilibrium position?

A chemical reaction is said to be at equilibrium when:

How does a reaction at equilibrium differ from a reaction that has reached completion?

Which statement accurately describes a system at dynamic equilibrium?

What does the equilibrium constant (K) indicate about a reversible reaction?

If a reaction has a very small equilibrium constant (K << 1), what does this imply about the reaction at equilibrium?

Consider the following reaction at equilibrium: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$. If, at equilibrium, the partial pressures are $P_{N_2} = 1 \text{ atm}$, $P_{H_2} = 2 \text{ atm}$, and $P_{NH_3} = 4 \text{ atm}$, what is the value of $K_p$?

For a certain reaction, the equilibrium constant $K_c$ is expressed using concentrations in molarity, while $K_p$ is expressed using partial pressures in atmospheres. Under what conditions are $K_c$ and $K_p$ equal for a given reaction?

Which of the following statements correctly describes the relationship between K, $K_c$, and $K_p$?

In what scenario is it possible to completely fill out an ICE table with numerical values directly from the information provided in the problem, without needing to solve for 'x'?

When using an ICE table to solve for equilibrium concentrations, under what circumstances would you include '0' as an initial concentration in the 'I' row?

How are stoichiometric coefficients used when completing the 'C' (Change) row of an ICE table?

What does it mean if the reaction quotient, Q, is much larger than the equilibrium constant, K ($Q >> K$)?

Which statement accurately describes the relationship between the reaction quotient (Q), the equilibrium constant (K), and the direction a reversible reaction will shift to reach equilibrium?

In the context of equilibrium calculations, what is the primary difference between using the equilibrium constant, K, and the reaction quotient, Q?

Consider the reaction $A + B \rightleftharpoons C + D$. At a certain point, $[A] = 2M$, $[B] = 1M$, $[C] = 3M$, and $[D] = 2M$. If the $K_c$ for this reaction is 4, which direction will the reaction shift to reach equilibrium?

Which of the following is a correct setup of an ICE table for the reaction $2A(g) \rightleftharpoons B(g)$, given an initial concentration of A as 2.0 M and no initial B, if 'x' represents the change in concentration of B?

For the reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, what expression correctly relates the changes in concentration of reactants and products in the 'C' row of an ICE table?

Given the initial concentrations $[A] = 2.0 M$ and $[B] = 0 M$ for the reaction $A(g) \rightleftharpoons 2B(g)$, and given the equilibrium constant $K = 4$, set up the correct equation to solve for 'x', where 'x' is the change in concentration of A.

Which of the following mathematical representations correctly describes how to calculate the equilibrium constant, K, for a given reversible reaction?

Consider the reversible reaction: $aA(g) + bB(g) \rightleftharpoons cC(g) + dD(g)$. Which expression correctly represents the equilibrium constant, $K_c$?

Which states of matter are excluded from the equilibrium constant expression ($K_c$) and why?

For the reversible reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, if at equilibrium there are significantly more reactants than products, what does this indicate about the value of $K_c$?

Given the reaction: $X(g) + 2Y(g) \rightleftharpoons Z(g)$ with an equilibrium constant $K_1$. If the reaction is reversed and multiplied by 2, resulting in $2Z(g) \rightleftharpoons 2X(g) + 4Y(g)$, how is the new equilibrium constant, $K_2$, related to $K_1$?

Consider two reactions: Reaction 1: $A(g) \rightleftharpoons B(g)$ with equilibrium constant $K_1$ Reaction 2: $B(g) \rightleftharpoons C(g)$ with equilibrium constant $K_2$. If the two reactions are added together, what is the equilibrium constant for the overall reaction $A(g) \rightleftharpoons C(g)$?

For the reaction $2NO(g) + O_2(g) \rightleftharpoons 2NO_2(g)$, $K_c$ is $4.0 \times 10^5$ at 25°C. If the reaction is written as $NO(g) + \frac{1}{2}O_2(g) \rightleftharpoons NO_2(g)$, what is the new value of $K_c$?

The equilibrium constant for the reaction $A(g) + B(g) \rightleftharpoons C(g)$ is $K$. If the concentrations of A, B, and C are all doubled, how is the reaction quotient, Q, related to K?

Consider the following sequential reactions: $A \rightleftharpoons B$ ($K_1 = 2$) and $B \rightleftharpoons C$ ($K_2 = 3$). What is the equilibrium constant for the overall reaction $A \rightleftharpoons C$?

When using ICE tables to solve equilibrium problems, what is the crucial difference between problems where you are given initial concentrations and K and asked to find equilibrium concentrations, versus problems where you are given some equilibrium concentrations and asked to find K?

Chemical Equilibrium

Equilibrium vs. Completion

At equilibrium, the rates are...

Dynamic Equilibrium

At equilibrium, the amounts are...

Equilibrium Constant (K)

K Value Significance

K, Kc, and Kp

ICE Table Method

Le Châtelier's Principle

Adding Reactant (Equilibrium)

Catalyst and Equilibrium

Equilibrium is Dynamic

K Expression

States Excluded from K

K and Product/Reactant Amounts

Multiplying a Reaction by a Coefficient

Reversing a Reaction

Adding Chemical Equations

What are ICE Tables?

Two Types of ICE Table Problems

Reaction Quotient (Q)

Manipulating K

Equilibrium Problem Type 1

Equilibrium Problem Type 2

Difference Between Type 1 and 2 Equilibrium Problems

Q < K

Q > K

ICE Table

ICE Table - Initial (I)

ICE Table - Change (C)

ICE Table - Equilibrium (E)