Notes

m1=m2 the mole concept formula...for isometric and adiabatic processes ,,,heat is minimal so the adiabatic curve is gonna be downwards........for isometric isothermal and isobariatic the curve is minimal ...r is directly proportional to 1 by root d....
Anachronism
An historically inaccurate detail in a literary work, included by the author either unintentionally or deliberately.
Saturated hydrocarbons are the simplest forms of hydrocarbons consisting entirely of single bonds that remain saturated with hydrogen atoms.

The general formula for acyclic saturated hydrocarbons or alkanes is CnH2n+2. The more general formula can also be written as CnH2n+2(1-r), where r is the number of rings.
Saturated hydrocarbons do not have any double or triple bonds between the carbon atoms in the structure, and all carbon atoms make four distinct covalent bonds.
The term saturated indicates the saturation of hydrogen atoms in the structure which also makes them the simples and least polar organic compounds.
Saturated hydrocarbons can occur either in a linear form or a branched form, depending on the complexity of the structure.
These hydrocarbons primarily occur in petroleum products as well as other forms of fossil fuels.
Saturated hydrocarbons burn with a blue, non-sooty flame which is why these are used as sources of fuel in vehicles and other engines.
Substitution reaction is the characteristic property of saturated hydrocarbons as they resist other reactions like hydrogenation and oxidative addition.
Saturated hydrocarbons have a lower concentration of carbon atoms as the number of hydrogen atoms is relatively high as compared to unsaturated hydrocarbons.
These are also more stable and less reactive and can resist attacks by nucleophiles and electrophiles.
Saturated hydrocarbons consist of two groups of hydrocarbon; acyclic alkanes and cycloalkanes.
Some examples of saturated hydrocarbons include methane, butane, propane, cyclohexane, etc. rms is equal to average and this is p average ....remem the formula and the relationship...vanderwall equation: unit of e and v ..comparison of gases on a and b...reduced form of vanderwall equation in specific conditions ..specific conditionds are very low pressure moderate pressure and then there is verified pressure ....3 conditions vanderwall conditions change...he mole concept is a convenient method of expressing the amount of a substance. Any measurement can be broken down into two parts – the numerical magnitude and the units that the magnitude is expressed in. For example, when the mass of a ball is measured to be 2 kilograms, the magnitude is ‘2’ and the unit is ‘kilogram’.

When dealing with particles at an atomic (or molecular) level, even one gram of a pure element is known to contain a huge number of atoms. This is where the mole concept is widely used. It primarily focuses on the unit known as a ‘mole’, which is a count of a very large number of particles.he number 6.02214076*1023 is popularly known as the Avogadro constant and is often denoted by the symbol ‘NA’. The elementary entities that can be represented in moles can be atoms, molecules, monoatomic/polyatomic ions, and other particles (such as electrons).

For example, one mole of a pure carbon-12 (12C) sample will have a mass of exactly 12 grams and will contain 6.02214076*1023 (NA) number of 12C atoms. The number of moles of a substance in a given pure sample can be represented by the following formula:

n = N/NA

Where n is the number of moles of the substance (or elementary entity), N is the total number of elementary entities in the sample, and NA is the Avogadro constant.

The word “mole” was introduced around the year 1896 by the German chemist Wilhelm Ostwald, who derived the term from the Latin word moles meaning a ‘heap’ or ‘pileThe number of moles of a molecule may not always be equal to the number of moles of its constituent elements. For example, a mole of water contains NA number of H2O molecules. However, each water molecule contains 2 hydrogen atoms and one oxygen atom. Therefore, one mole of H2O contains 2 moles of hydrogen and one mole of oxygen.


Related Quantities and their Formulae
Atomic and Molecular Mass
The atomic mass of an element is the mass of one atom of the element expressed in atomic mass units (amu). It accounts for the abundance of the various isotopes of the element and assigns an average value to the mass of one atom of the element.

For example, the atomic mass of carbon is 12.011 atomic mass units since carbon samples generally contain 98.89% of the carbon-12 isotope, 1.11% of carbon-13, and trace amounts of carbon-14. However, the atomic masses of these isotopes are different.

The atomic mass of a carbon-12 atom is 12 atomic mass units, but that of a carbon-13 atom is 13 amu. The atomic mass of an element is roughly equal to the sum of all the protons and neutrons present in its nucleus.

The molecular mass of an element is the sum of the atomic masses of all its constituent elements. This quantity is also represented in terms of atomic mass units. Therefore, the molecular mass of water is equal to the sum of the atomic masses of its constituents – hydrogen and oxygen.

The atomic mass of hydrogen is 1.00794 amu and that of oxygen is 15.9994. Since water molecules contain 2 hydrogen atoms and only one oxygen atom, the molecular mass of H2O is 18.0154 amu.

Molar Mass
The molar mass of a substance is defined as the total mass of one mole of the substance. It is often represented in terms of ‘grams per mole’ (g/mol). However, the SI unit of this quantity is kg/mol. Molar mass can be represented by the following formula:

Molar mass of a Substance = (Mass of the Substance in grams)/(Number of Moles)

For example, the molar mass of water is approximately 18.015 g/mol, which is the mass of NA number of water molecules.

Gram Atomic Mass and Gram Molecular Mass
The gram atomic mass of an element is the mass of one mole of that element. Similarly, the gram molecular mass of a compound refers to the mass of a single mole of the compound. Therefore, the gram atomic mass of hydrogen is approximately 1.007g and the gram molecular mass of water is approximately 18.015g.