2. Atoms & Elements

Law of Definite Proportions

Law of Definite Proportions   Chemistry Made Easy

Law of Constant Proportions | Don't Memorise

Proust's Law (Law of Definite Proportions)

How many hydrogen atoms are in each of the following: 
(b) Ca1C2H5COO22?

Upon decomposition, one sample of magnesium fluoride produces
1.65 kg of magnesium and 2.57 kg of fluorine. A second
sample produces 1.32 kg of magnesium. How much fluorine (in
grams) does the second sample produce?

Determine the number of each type of atom in each formula.
b. CuSO4

A chemist finds that 30.82 g of nitrogen will react with 17.60,
35.20, 70.40, or 88.00 g of oxygen to form four different
compounds. (a) Calculate the mass of oxygen per gram of
nitrogen in each compound. 30.82 g N and 70.40 g O

A 7.83 g sample of HCN contains 0.290 g of H and 4.06 g of N.
Find the mass of carbon in a sample of HCN with a mass of 3.37 g.

The chloride of an unknown metal is believed to have the formula
MCl3. A 2.395-g sample of the compound contains
3.606 * 10 - 2 mol Cl. Find the atomic mass of M.

Determine the number of each type of atom in each formula.
c. Al(NO3)3

The mass ratio of sodium to fluorine in sodium fluoride is
1.21:1. A sample of sodium fluoride produces 28.8 g of sodium
upon decomposition. How much fluorine (in grams) forms?

Law of: Definite Proportions vs Multiple Proportions vs Conservation of Mass

A chemist finds that 30.82 g of nitrogen will react with 17.60,
35.20, 70.40, or 88.00 g of oxygen to form four different
compounds. (a) Calculate the mass of oxygen per gram of
nitrogen in each compound. 30.82 g N and 17.60 g O

A 1.0-g sample of carbon dioxide (CO2) is fully decomposed
into its elements, yielding 0.273 g of carbon and 0.727 g of
oxygen. (a) What is the ratio of the mass of O to C?

A chemist finds that 30.82 g of nitrogen will react with 17.60,
35.20, 70.40, or 88.00 g of oxygen to form four different
compounds. (a) Calculate the mass of oxygen per gram of
nitrogen in each compound. 30.82 g N and 35.20 g O

A chemist finds that 30.82 g of nitrogen will react with 17.60,
35.20, 70.40, or 88.00 g of oxygen to form four different
compounds. (a) Calculate the mass of oxygen per gram of
nitrogen in each compound. 30.82 g N and 88.00 g O

Law of Definite Proportions Example 1

Law of Definite Proportions Example 2

ChemLab - 2. The Law of Definite Proportions

Two samples of carbon tetrachloride are decomposed into their
constituent elements. One sample produces 38.9 g of carbon
and 448 g of chlorine, and the other sample produces 14.8 g of
carbon and 134 g of chlorine. Are these results consistent with
the law of definite proportions? Explain your answer.

A 7.74 g sample of HCN is found to contain 0.287 g of H and 4.01 g N. Find the mass of carbon in a sample of HCN with a mass of 3.43 g.

How many of the indicated atoms are represented by each
chemical formula: (a) carbon atoms in C4H9COOCH3

Determine the number of each type of atom in each formula.
a. Ca(NO2)2

A sample of ascorbic acid (vitamin C) is synthesized in
the laboratory. It contains 1.50 g of carbon and 2.00 g of
oxygen. Another sample of ascorbic acid isolated from
citrus fruits contains 6.35 g of carbon. According to the
law of constant composition, how many grams of oxygen
does it contain?

Chemistry 5.8a Law of Definite Proportions

How many of the indicated atoms are represented by each 
chemical formula: (b) oxygen atoms in Ca1ClO322

Write a ratio showing the relationship between the molar
amounts of each element for each compound. (See Appendix
IIA for color codes.)
(a) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/15329094dccffcc3-1659717849693.jpg" alt="" />

Law of Definite Proportions - Law of multiple proportions

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1. Intro to General Chemistry

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

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Millikan Oil Drop Experiment

The Oil Drop Experiment helped with determining the fundamental charge of the electron.&nbsp;

Ions

Ions represent elements that possess either a positive charge or a negative charge.&nbsp;

Periodic Table: Charges

Elements lose or gain electrons to have the ideal number of outer shell electrons like the noble gases.&nbsp;

"Different samples of a pure chemical compound always contain the same proportions of elements by mass."

Periodic Table: Classifications

The Periodic Table contains 3 Major Classifications when describing its elements

Isotopes

Isotopes are atoms of an element that have the same atomic number, but different mass number.&nbsp;

The Atom

The atom represents the basic functional unit in chemistry

Mole Concept

The Mole Concept involves the interconversions between different unit amounts of a substance.

Periodic Table: Representative Elements & Transition Metals

The Groups of the Periodic Table can be broken down into the Representative Elements and Transition Metals

Atomic Theory

John Dalton, one of the "Fathers of Chemistry"is credited with modernizing the Atomic Theory.

Subatomic Particles

The atom is composed of 3 subatomic particles:neutrons, protons, and electrons.

Periodic Table: Elemental Forms

The elements of the Periodic Table exist in different elemental forms in the natural world

Periodic Table: Phases

Under standard conditions of temperature and pressure, the elements can exist as solids, liquids or gases

Atomic Mass

The atomic mass of an element includes the masses of all 3 subatomic particles of neutrons, protons and electrons.&nbsp;

Periodic Table: Group Names

The Periodic Table can be further classified into Periods and Groups.&nbsp;

Law of Conservation of Mass

"In a chemical reaction, no matter is created or destroyed, but instead changes form."

Calculating Molar Mass

Molar Mass is a physical property that represents the mass of a substance divided by the amount of that substance.

Rutherford Gold Foil Experiment

The Gold Foil Experiment helped with the discovery of the positively charged nucleus.

Law of Multiple Proportions

“When 2 elements (A &amp; B) form different compounds, the mass of Element B that combine with 1 g of A are a ratio of whole numbers."

Periodic Table: Element Symbols

The Element Symbols of the Periodic Table represent the abbreviated form of an element