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A chemical reaction is a process that results in the interconversion of chemical substances.The substance or substances initially involved in a chemical reaction are called reactants.Classically, chemical reactions encompass changes that strictly involve the motion of electrons in the forming and breaking of chemical bonds, although the general concept of a chemical reaction, in particular the notion of a chemical equation, is applicable to transformations of elementary particles, as well as nuclear reactions.

Reaksi kimia adalah transformasi/perubahan dalam struktur molekul. Reaksi ini bisa menghasilkan penggabungan molekul membentuk molekul yang lebih besar, pembelahan molekul menjadi dua atau lebih molekul yang lebih kecil, atau penataulangan atom-atom dalam molekul. Reaksi kimia selalu melibatkan terbentuk atau terputusnya ikatan kimia

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On the classical definition, therefore, there are only two types of chemical reaction: redox reactions and acid-base reactions. The former involve the motion of lone electrons and the latter of an electron pair.

Chemical reactions may be classified in different ways depending on the particular aspect considered for elaborating the division, or on the branch of Chemistry which the classification originates from. Some examples of widely used terms for describing common kinds of reactions are:

Isomerisation, in which a chemical compound undergoes a structural rearrangement without any change in its net atomic composition; see stereoisomerism

Direct combination or synthesis, in which two or more chemical elements or compounds unite to form a more complex product:

Chemical decomposition or analysis, in which a compound is decomposed into smaller compounds or elements:

Single displacement or substitution, characterized by an element being displaced out of a compound by a more reactive element:

Double displacement or coupling substitution, in which two compounds in aqueous solution (usually ionic) exchange elements or ions to form different compounds:

Combustion, in which any combustible substance combines with an oxidizing element, usually oxygen, to generate heat and form oxidized products. The term combustion is used usually only large-scale oxidation of whole molecules, i.e. a controlled oxidation of a single functional group is not combustion.

Soal Kimia

berikut adalah soal latihan kimia yang lebih di tekankan pada pemahaman terhadap reaksi kimia, meliputi entalphi, reaksi molar, enerigi ikatan dan panas pembakaran. soal dalam bahasa indonesia, dengan format dokumen berupa pdf.

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Soal tersebut dalam bentuk pilihan ganda yang di sesuaikan dengan format soal SPMB dan soal UAN, sehingga diharapkan memudahkan para siswa untuk belajar, Soal lainya akan kami usahakan secepatnya, Selamat Belajar

In chemistry, colligative properties are the properties of dilute solutions of non-volatile solutes whose values depend only on the concentration of solute particles, not on the type of particles present.
Sifat koligatif larutan adalah sifat larutan yang tidak tergantung pada macamnya zat terlarut tetapi semata-mata hanya ditentukan oleh banyaknya zat terlarut (konsentrasi zat terlarut).

The four colligative properties are:

Vapor pressure depression: The change in vapor pressure where the solute is less volatile than the solvent is regulated by Raoult’s law, which states that the pressure is equal to the mole fraction of the solvent times the vapor pressure of pure solvent: P = Xsolvent*P°. This holds truest for ideal solutions.

Freezing-point depression: The presence of a solute decreases the freezing point as compared to a pure solvent. The exact change (?T) can be calculated as van ‘t Hoff factor (i) of the solute multiplied by its molality (m) multiplied by the freezing point depression constant of the solvent (Kf): ?T = i(?Kf)m. Alternatively, it can be calculated as the total molality of all solutes in solution times the depression constant: ?T = Kf ? m.

Boiling-point elevation: Because of the lowered vapor pressure, the boiling point of a solution is elevated as compared to the pure solvent. The change in boiling point (?T) can be calculated in the same way as the change in freezing point, except a different constant is used: the van ‘t Hoff factor (i) of the solute multiplied by its molality multiplied by the boiling point elevation constant of the solvent (Kb): ?T = iKbm. ?T can also be calculated using the sum of all molalities: ?T = Kb ? m.

Osmotic pressure: The presence of solute can cause pressure to be exerted across a permeable membrane according to an equation quite similar to the ideal gas law: ? is the osmotic pressure, n is the number of moles of solute, R is the ideal gas constant, T is the absolute temperature in kelvins, and V is the volume: ? = (nRTi)/V.

Sifat koligatif meliputi:

1. Penurunan tekanan uap jenuh
2. Kenaikan titik didih
3. Penurunan titik beku
4. Tekanan osmotik

Banyaknya partikel dalam larutan ditentukan oleh konsentrasi larutan dan sifat Larutan itu sendiri. Jumlah partikel dalam larutan non elektrolit tidak sama dengan jumlah partikel dalam larutan elektrolit, walaupun konsentrasi keduanya sama. Hal ini dikarenakan larutan elektrolit terurai menjadi ion-ionnya, sedangkan larutan non elektrolit tidak terurai menjadi ion-ion. Dengan demikian sifat koligatif larutan dibedakan atas sifat koligatif larutan non elektrolit dan sifat koligatif larutan elektrolit.
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Soal tersebut dalam bahasa indonesia dengan format pdf, berbentuk pilihan ganda di sesuaikan dengan format soal UAN dan SPMB