TRAINING REQUIREMENT CHEMISTRY 1

The course aims to provide the fundamentals of stoichiometry and the basic definitions of General Chemistry, serving as a prerequisite for the study of the subject. In particular, through the study of stoichiometry and basic nomenclature, students will acquire fundamental concepts regarding the structure of matter in its various states of aggregation, with a specific focus on chemical substances and compounds. Students will be required to perform the stoichiometric calculations that underpin chemical measurements.

The course includes 14 hours of lectures dedicated to working through exercises useful for solving the written exam.

Basic mathematics, basic physics, and basic chemistry. The OFA course does not require extensive prior knowledge; however, it is essential to keep up with the various topics as they are presented and not fall behind in your studies. Chemistry is a cumulative subject, and it is impossible to grasp the material without regular, consistent study throughout the course. It will be very difficult to prepare for the exam on your own at the end of the course, as many topics require time to be fully understood and assimilated.

Mandatory for students with OFAs. Strongly recommended for all others. Class attendance will contribute positively to the student's assessment.

STOICHIOMETRY - Atoms and molecules - Mixtures and compounds - Atomic number, mass number - Isotopes - Atomic mass unit - Basic nomenclature - The concept of the mole - Laws of stoichiometry - Determination of a compound's formula – Atomic weight and molecular weight - The chemical equation and its balancing - Stoichiometric calculations: quantitative relationships in chemical reactions – Limiting reactant - Numerical applications

1.CHEMICAL PRINCIPLES - Atkins, Jones, Laverman

2. Stoichiometry- B I Bhatt-S B Thakore

3. Chemical Reactions and Stoichiometry, R. K. Dave

4. Chemistry: A Molecular Approach (5th edition) Nivaldo J. Tro, Global Edition

5. Chemistry & Chemical Reactivity. Kotz/Treichel/Townsed

Lecture notes

A written assignment with simple stoichiometry and nomenclature exercises.

1) Write the formulas for the following compounds:

Hydrochloric acid, periodic acid, potassium sulfide, sodium sulfate, cesium nitrite.

 

2) Calculate the mass in grams of sodium and nitrogen present in 15.30 g of NaNO₃. (Atomic mass Na = 22.99 amu, N = 14.01 amu; O = 16.00 amu).

 

3) A chlorinated organic compound with the formula CxHyOzClw yielded the following results upon elemental analysis: %C = 44.17%, %H = 2.51%, %O = 9.86%. Calculate the empirical formula of the compound. (Atomic mass C = 12.01 amu, H = 1.01 amu; O = 16.00 amu; Cl = 35.45 amu).

 

4) Calculate the molarity of an HCl solution obtained by mixing 4.00 mL of a 1.20 × 10⁻² M HCl solution with 2.00 mL of a 1.00 × 10⁻² M HCl solution.

 

5) 1.40 moles of SrO react with 3.35 moles of water to produce Sr(OH)₂ according to the reaction:

SrO + H₂O → Sr(OH)₂

Calculate the mass in grams of Sr(OH)₂ produced at the end of the reaction.

(Atomic mass Sr = 87.72 amu, H = 1.008 amu, O = 16.00 amu)

 

6) Explain the difference between a mixture and a compound.