Some Basic Concepts of Chemistry Shobhit Nirwan

36 grams of water.

A reactant which gets converted and limits the amount of product formed.

7

The mass of one mole of an ionic compound in grams.

Mass percent = mass of solute/mass of solution × 100.

M1V1 = M2V2

Molarity (M) = no. of moles of solute / volume of solution in litres

Molality = No. of moles of solute / Mass of solvent in kg

No, the molality of a solution does not change with temperature.

Mass (kilogram), volume (cubic meter), density (kilogram per cubic meter), temperature (kelvin).

Chemical change.

Mass percent, mole fraction, molarity, molality.

Substances with components in fixed composition that cannot be separated.

Properties that can be observed or measured without changing the composition of the substance.

CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (g)

Dihydrogen (H2).

It is raised by 1.

The mass of one mole of a substance in grams.

Results must be reported with no more significant figures than are there in the measurement with few significant figures.

Antoine Lavoisier.

Five O2 molecules.

Joseph Proust.

1. Matter consists of indivisible atoms. 2. All the atoms of a given element have identical properties including identical mass. Atoms of different elements differ in mass. 3. Compounds are formed when atoms of different elements combine in a fixed ratio. 4. Chemical reactions involve reorganization of atoms, which are neither created nor destroyed in a chemical reaction.

Cisplatin, Taxol, and AZT (Azidothymidine).

2.32508 × 10^2.

Exactly 1/12 of the mass of one carbon-12 atom.

By adding the atomic masses of the elements present in the compound.

a × 10^b, where 'a' is a number between 1 and 10, and 'b' is a positive or negative exponent.

By dividing the mass of that element in the compound by the molar mass of the compound and multiplying by 100.

If 2 elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.

Matter can neither be created nor destroyed.

Law of conservation of mass, law of definite properties, law of multiple proportions, Gay Lussac’s Law of gaseous volumes, Avogadro Law.

It is a convenient method of expressing the amount of a substance.

Particles are held close, have definite volume and shape.

Amount of mass per unit volume.

Sodium, copper, oxygen.

By multiplying the atomic mass of each element by their respective number of atoms and then adding the results together.

A balanced chemical equation has the same number of atoms of each element on both sides of the equation.

10%.

By placing the coefficient 5 on the left of oxygen on the left side of the equation.

Carbon dioxide (CO2) and water (H2O).

A solution of known higher concentration used to prepare solutions of desired concentration by dilution.

A theory that states that matter is composed of small, indivisible particles called atoms.

General conference on weights and measures.

Mass is the amount of matter present, while weight is the force exerted by gravity on an object.

A mixture where components do not mix completely and the composition is not uniform.

Atomic masses are based on carbon-12 as the standard.

By comparing the amount of each reactant to the stoichiometry of the balanced equation.

Ensure the powers of 10 are equal before performing the operation.

5 is simply dropped.

Round 'a' to the nearest order of magnitude, i.e., 'b' is also c/d order of magnitude.

Solid, liquid, gas.

Dalton.

Color, odor, melting point, boiling point, and density.

The calculation of quantities of reactants and products in chemical reactions.

Particles are close, can move around, have definite volume but not definite shape.

Degree Celsius, degree Fahrenheit, Kelvin.

0.5 moles of methane.

By using the moles of the limiting reagent and the stoichiometry of the balanced equation.

By trial and error.

The ratio of the number of moles of a particular component to the total number of moles of the solution.

The exact number of different atoms present in a molecule of a compound.

Homogeneous mixtures and heterogeneous mixtures.

Elements and compounds.

Gay Lussac.

Acidity, basicity, combustibility.

A mixture where components completely mix with each other and the composition is uniform.

Add exponents for multiplication, subtract exponents for division.

38.64 × 10^13 or 3.864 × 10^14

1. All non-zero digits are significant. 2. All zeroes between non-zero digits are significant. 3. Trailing zeroes in a number without a decimal point are not significant.

4 Fe(s) + 3O2(g) → 2Fe2O3(s)

It is the number of moles of the solute in 1 litre of the solution.

200 ml of 1 M NaOH is taken and enough water is added to dilute it to make it 1 litre.

When gases combine or are produced in a chemical reaction, they do so in a simple ratio by volume provided all gases are at the same temperature & pressure.

Physical properties and chemical properties.

Equal volumes of gases at the same temperature and pressure should contain an equal number of molecules.

Weather patterns, functioning of brain, and operation.

Metre, kilogram, second, ampere, Kelvin, mole, candela.

Particles are far apart, movement is easy and fast, and they have neither definite volume nor definite shape.

1.6 × 10^-4.

The amount of a substance that contains as many particles or entities as there are atoms in exactly 12g of the 12C isotope.

The result cannot have more digits to the right of the decimal point than either of the original numbers.

The simplest whole number ratio of different atoms present in a compound.

A given compound always contains exactly the same proportion of elements by weight.

Avogadro.

Fertilizers, acids, salts, dyes, polymers, drugs, and soaps.

Using an analytical balance.

A substance whose constituents cannot be separated into simpler substances by physical methods, but can be separated by chemical methods.