Question 10.4: Reversible Reactions and Equilibrium Complete each of the fo...

Chemistry an Introduction to General, Organic, and Biological Chemistry

Reversible Reactions and Equilibrium

Complete each of the following with equal or not equal, faster or slower, change or do not change:

a. Before equilibrium is reached, the concentrations of the reactants and products ——————.

b. Initially, reactants have a —————— rate of reaction than the rate of reaction of the products.
c. At equilibrium, the rate of the forward reaction is —————— to the rate of the reverse reaction.

d. At equilibrium, the concentrations of the reactants and products ——————.

The blue check mark means that this solution has been answered and checked by an expert. This guarantees that the final answer is accurate.
Learn more on how we answer questions.

Related Answered Questions

Question: 10.13

Identifying Buffer Solutions Indicate whether each of the following would make a buffer solution: a. HCl, a strong acid, and NaCl b. H3PO4, a weak acid c. HF, a weak acid, and NaF ...

Verified Answer:

a. No. A buffer requires a weak acid and a salt co...

Question: 10.12

Titration of an Acid A 25.0-mL (0.025 L) sample of an HCl solution is placed in a flask with a few drops of phenolphthalein (indicator). If 32.6 mL of a 0.185 M NaOH solution is needed to reach the endpoint, what is the molarity of the HCl solution? NaOH(aq) + HCl(aq) → H2O(l) + NaCl(aq) ...

Verified Answer:

Step

\fbox{1}

State the given and...

Question: 10.8

Calculating pH from [H3O^+] Aspirin, which is acetylsalicylic acid, was the first nonsteroidal anti-inflammatory drug used to alleviate pain and fever. If a solution of aspirin has a [H3O^+] = 1.7 × 10^-3 M, what is the pH of the solution? ...

Verified Answer:

Step

\fbox{1}

State the given and...

Question: 10.5

Effect of Changes in Concentration on Equilibrium An important reaction in the body fluids is H2CO3(aq) + H2O(l) ←→ HCO3^-(aq) + H3O^+(aq) Use Le Châtelier’s principle to predict whether the system shifts in the direction of products or reactants for each of the following: a. adding some H2CO3(aq) ...

Verified Answer:

According to Le Châtelier’s principle, when stress...

Question: 10.2

Acids and Bases In each of the following equations, identify the reactant that is a Brønsted–Lowry acid and the reactant that is a Brønsted–Lowry base: a. HBr(aq) + H2O(l) → Br^-(aq) + H3O^+(aq) b. CN^-(aq) + H2O(l) ←→ HCN(aq) + OH^-(aq) ...

Verified Answer:

a. HBr, acid;

H_{2} O

, base b. [lat...

Question: 10.11

Balancing Equations of Acids Write the balanced equation for the neutralization of HCl(aq) and Ba(OH)2(s). ...

Verified Answer:

Step

\fbox{1}

Write the reactants...

Question: 10.10

Equations for Metals and Acids Write a balanced equation for the reaction of Al(s) with HCl(aq). ...

Verified Answer:

Write the reactants and products. When a metal rea...

Question: 10.9

Calculating [H3O^+] from pH Determine the [H3O^+] for solutions having each of the following pH values: a. pH = 3.0 b. pH = 8.25 ...

Verified Answer:

a. For pH values that are whole numbers, the [late...

Question: 10.7

pH of Solutions Consider the pH of the following items: ...

Verified Answer:

a. The most acidic item is the one with the lowest...

Question: 10.6

Calculating the [H3O^+] of a Solution A vinegar solution has a [OH^-] = 5.0 × 10^-12 M at 25 °C. What is the [H3O^+] of the vinegar solution? Is the solution acidic, basic, or neutral? ...

Verified Answer:

Step

\fbox{1}

State the given and...