Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

6. Chemical Reactions & Quantities

Stoichiometry

GOB Chemistry

6. Chemical Reactions & Quantities

Stoichiometry

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2:12 minutes

Problem 8a

Textbook Question

Balance the following equation, and tell how many moles of nickel will react with 9.81 mol of hydrochloric acid.
Ni(s) + HCl(aq) → NiCl₂(aq) + H₂(g)

Verified step by step guidance

Write the unbalanced chemical equation:

Ni (s) + {HCl}_{(aq)} \to {NiCl}_{2 (aq)} + H_{2 (g)}

Balance the equation by ensuring the number of atoms of each element is the same on both sides. Start with nickel (Ni), which is already balanced. Then balance chlorine (Cl) by placing a coefficient of 2 in front of HCl. Finally, balance hydrogen (H) by ensuring there are 2 H atoms on both sides of the equation. The balanced equation is:

Ni (s) + 2 {HCl}_{(aq)} \to {NiCl}_{2 (aq)} + H_{2 (g)}

Identify the mole ratio between nickel (Ni) and hydrochloric acid (HCl) from the balanced equation. The ratio is 1 mol of Ni to 2 mol of HCl.

Use the given amount of HCl (9.81 mol) to calculate the moles of Ni required. Apply the mole ratio:

\frac{1}{2}

(1 mol Ni / 2 mol HCl). Set up the calculation as:

9.81 \times \frac{1}{2}

Simplify the calculation to determine the moles of nickel (Ni) that will react with 9.81 mol of HCl. This will give you the final answer.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining how many moles of one substance will react with a given amount of another.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is crucial because it reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. A balanced equation provides the correct stoichiometric ratios needed to calculate the moles of reactants and products.

Mole Concept

The mole concept is a fundamental principle in chemistry that defines a mole as a specific quantity of particles, typically 6.022 x 10^23 (Avogadro's number). It allows chemists to convert between the mass of a substance and the number of particles or moles. Understanding the mole concept is vital for performing calculations involving the amounts of reactants and products in chemical reactions.

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Related Practice

Multiple Choice

The oxidation of chromium solid is represented by the following equation:

4 Cr (s) + 3 O₂ (g) → 2 Cr₂O₃ (s)

How many moles of chromium (III) oxide are produced when 34.69 g Cr reacts with excess oxygen gas?

The reaction of potassium chlorate and sucrose is given below:

8 KClO₃ + C₁₂H₂₂O₁₁ → 8 KCl + 12 CO₂ + 11 H₂O

If 2.33 x 10^-7 formula units of potassium chlorate are reacted, how many grams of carbon dioxide will be produced?

If the density of ethanol, CH₃CH₂OH, is 0.789 g/mL, how many milliliters of ethanol are needed to produce 4.8 g of H₂O in the following reaction?

CH₃CH₂OH (l) + 3 O₂ (g) → 3 H₂O (l) + 2 CO₂ (g)

How many moles of NiCl₂ can be formed in the reaction of 6.00 mol of Ni and 12.0 mol of HCl?

Ni(s) + HCl(aq) → NiCl₂(aq) + H₂(g)

1522

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Textbook Question

The following diagram represents the reaction of A₂(red spheres) with B₂(blue spheres):

<IMAGE>

b. How many moles of product can be made from 1.0 mol of A₂? From 1.0 mol of B₂?

1373

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Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

a. Write mole ratios to show the relationship between the reactants and products for each reaction.

1659

views

Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

c. How many kilograms of rutile are needed to produce 95 kg of Ti?

1427

views

Textbook Question

Titanium metal is obtained from the mineral rutile, TiO2. The process requires multiple steps, as shown in the following reactions:

TiO₂(s) + 2 Cl₂(g) + 2 C(s) → TiCl₄(s) + 2 CO(g)

TiCl₄(s) + 2 Mg(s) → Ti(s) + 2 MgCl₂(s)

b. How many moles of TiO2 are needed to form one mole of titanium?

1738

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Balance the following equation, and tell how many moles of nickel will react with 9.81 mol of hydrochloric acid.Ni(s) + HCl(aq) → NiCl2(aq) + H2(g)

Key Concepts

Stoichiometry

Balancing Chemical Equations

Mole Concept

Watch next

Balance the following equation, and tell how many moles of nickel will react with 9.81 mol of hydrochloric acid.
Ni(s) + HCl(aq) → NiCl₂(aq) + H₂(g)