A molecule of Sulphuric Acid, H2SO4, consists of two atoms of hydrogen, one atom of sulphur and four atoms of oxygen
Sulphuric acid is a colourless viscous corrosive oily liquid, which has
Sulphuric acid is the strong acid produced by dissolving sulphur trioxide in water.
SO3 + H2O ==> H2SO4
The Strength of Acids is determined by the degree to which they are ionised in aqueous solution.
For example, Sulphuric Acid, H2SO4, which is a strong acid is fully dissociated, and all the displaceable hydrogen in the acid is present in solution as Hydrogen Ion, H(+). H2SO4 ==> H(+) + SO4
100% as H(+)
In contrast, the weak acids ethanoic acid, CH3COOH, is partially ionised in solution, and only approximately 5% of the displaceable Hydrogen in the acid is present in solution as hydrogen ion, H(+).
Preparation of Sulphuric AcidCombustion of Sulphur
When a small amount of Sulphur, S, is kindled on a deflagrating spoon, it burns with a bright blue flame when introduced into a gas jar containing Oxygen, O2. A gas, Sulphur Dioxide, SO2, is the main product of the combustion. However, a little Sulphur Trioxide, SO3, is also formed, which makes the gas slightly cloudy.
S + O2 ==> SO2
Sulphur Dioxide
2S + 3O2 ==> 2SO3
Sulphur Trioxide
When shaken with water, the products of combustion dissolve, forming an acidic solution which turns litmus red.
Reactions of Sulphuric acidElectrolysis of a Solution of dilute Sulphuric Acid
The Electrolysis of an Aqueous Solution of dilute Sulphuric Acid is often carried out in a Hofmann Voltammeter, an apparatus in which the gases evolved at the anode and cathode can be collected in separate graduated tubes. When the solution is electrolyzed hydrogen is produced at the cathode and oxygen at the anode. These gases can be shown to be present in a 2 to 1 ratio and result from the electrolysis of water under acidic conditions.
Sulphuric acid is a strong electrolyte is fully dissociated in aqueous solution.
H2SO4 ==> 2 H(+) + SO4(2 -) Water is a weak electrolyte and is only slightly dissociated H2O ==> H(+) + OH(-) During electrolysis, the Hydrogen Ions, H(+), migrates towards the cathode, and are discharged there (i.e. they gain an electron and are converted to hydrogen gas). 2 H(+) + 2 e(-) ==> H2-
At the anode the concentration of Hydroxyl Ions, HO(-),is too low to maintain a reaction and the Sulphate Ions, SO4(2 -) are not oxidized but remain on in solution at the end. Water molecules must be the species reacting at the anode.
2 H2O ==> O2 + 4 H(+) + 4 e(-)
The overall reaction is
Cathode Reaction :
2 H(+) + 2e(-) ==> H2 4 H(+) + 4e(-) ==> 2H2
Anode Reaction :
2 H2O ==> O2 + 4 H(+) + 4 e(-)
Overall Cell Reaction:
4 H(+) + 2 H2O ==> 2 H2 + O2 + 4 H(+)
For every Hydrogen Ions, H(+), discharged at the anode, another hydrogen ion is formed at the cathode. The net result is that the concentration of the Sulphuric Acid, H2SO4, remains constant and this electrolysis consists of the decomposition of water with the overall reaction
2H2O ==> 2H2- + O2-
Ferrous Sulphate, Fe(II)SO4, is the salt formed when Iron, Fe, is dissolved in Sulphuric Acid, H2SO4.
Hydrogen Chloride, HCl, may be prepared in the laboratory by heating Concentrated Sulphuric Acid, H2SO4, with Sodium Chloride, NaCl.
NaCl + H2SO4 ==> NaHSO4 + HCl
Many Metallic Chlorides liberate Chlorine, Cl2, when treated with Sulphuric Acid, H2SO4, and Manganese Dioxide, MnO2).
Many Metallic Chlorides liberate Hydrogen Chloride gas, HCl, when warmed with concentrated Sulphuric Acid, H2SO4.
Sulphur Trioxide, SO3, is prepared by heating concentrated Sulphuric Acid, H2SO4, with a large excess of Phosphorus Pentoxide, P2O5.
H2SO4 + P2O5 ==> SO3 + 2 HPO3
Sulphur Dioxide, SO2, is usually made in the laboratory by heating concentrated Sulphuric Acid, H2SO4, with Copper turnings, Cu.
Cu + 2 H2SO4 ==> CuSO4 + SO2 + 2 H2O
Hydrogen Fluoride, HF, can be prepared in the laboratory by heating Concentrated Sulphuric Acid, H2SO4, with Calcium Fluoride, CaF2.
H2SO4 + CaF2 ==> 2 HF + CaSO4
Hydrogen Iodide, HI, can be prepared by direct combination of the elements using a platinum catalyst. In the laboratory it is prepared by heating Concentrated Sulphuric Acid, H2SO4, with Sodium Iodide, NaI.
H2SO4 + 2 NaI ==> 2 HI + Na2SO4
Methanol, CH3OH, does not undergo dehydration reactions. Instead, in reaction with Sulphuric Acid, H2SO4, the ester, Dimethyl Sulphate, (CH3)2SO4, is formed.
concentrated H2SO4 2CH3OH ==> (CH3)2SO4 + H2O Methanol Dimethyl Water Sulphate
Sulphuric Acid, H2SO4, absorbs Ethylene, C2H4, at room temperature to form Ethyl Hydrogen Sulphate, C2H5.HSO4, with much evolution of heat.
C2H4 + H2SO4 ==> C2H5.HSO4
If this is treated with Water, H2O and warmed, Ethanol, C2H5OH, is formed.
heat C2H5.HSO4 + H2O ==> C2H5OH + H2SO4
Zinc, Zn, is a transition metallic element found in Group IIb of the Periodic Table.
Zinc was known from ancient times, when Brass (i.e. an alloy of Copper and Zinc) was used. Lohneyes was the first to apply the term "Zinc" correctly to the metal that we know today in 1697AD.
OccurrenceZinc is found in different ore forms, including
Zinc is extracted using two process :
Zn + H2SO4 ==> ZnSO4 + H2
Zn + 2 NaOH ==> Na2ZnO2 + H2
UsesZinc is in widespread useIt's FeS, iron and sulphur, Fe & S
Chemical reaction is the making and breaking of chemical bonds, leading to changes in the composition of matter. Chemical reactions do not create or destroy matter; they only rearrange it in various ways.
The products of making a chemical reaction is bakingsoda and vinger.Mix them together then you have a chemicle reaction
Bonds in the reactants are broken, and bonds in the product are formed.
Because at higher temperatures, there is more energy in the reactants. With more energy, they move faster. This makes them more likely to collide, causing a chemical reaction. This also results in more energy at the impact, making it easier and more likely that the reactants achieve the activation energy required for the reaction to happen. Also, in decomposition reactions, there is more energy available to complete the reaction, and the "binding states" of the reactants are under more stress (so they are easier to "break").
When producing ammonia, there is not a 100% change from reactants into products. In fact, around half of the reactants will change into ammonia, and then equilibria is reached and the amount of ammonia will stay the same. Increasing the pressure shifts the equilibria, so that more ammonia is produced when an equilibria is reached, making the process more efficient. Hypothetical example: 1 litre of reactants (normal pressure) -----> 0.5 litre reactants and 0.5 litre ammonia 1 litre of reactants (high pressure) -------> 0.2 litre reactants and 0.8 litre ammonia
Chemical reaction is the making and breaking of chemical bonds, leading to changes in the composition of matter. Chemical reactions do not create or destroy matter; they only rearrange it in various ways.
By making interact under certain conditions of temperature, pressure, concentration, etc. the reactants.
Chemical reactions always involve changes in the chemical bonds that join atoms in compounds. At least one chemical bond is broken or formed during a chemical reaction.
Bonds are both broken and made in an exothermic reaction, but in the end, the potential chemical energy of the products is less than the potential chemical energy of the reactants.
Yes, it is a chemical reaction.
Toasting bread is a chemical reaction.
The more concentrated the solution of reactants, the more the reaction wants to push right making more products.Same goes vice-versa; if there's more products, then the reaction will push left producing more reactants.
Chemical reactions are driven by the amount of energy used to break the bonds in the reactants ( the activation energy) and the energy released by making new bonds in the products. The stronger the forces holding together the molecules of products, the more readily the reaction takes place. The difference between the energy produced in making the bonds and breaking the bonds is called ENTHALPY. The reaction can also be driven if the products have a greater degree of disorder (ENTROPY) than the reactants.
Energy is only released when chemical bonds are formed. ... This balanced chemical equation summarizes the chemical reaction involved in burning methane. The reactants are on the left, the products are on the right, and the arrow ... in making carbon dioxide and water is used to break more bonds in the ...
In a chemical reaction, reactants and products are different substances, but they're made up of the same atoms. The law of conservation of matter says that matter cannot be created or destroyed. So, the matter that makes up the reactants (what you have before the reaction) is the same matter that makes up the products (what you get at the end of the reaction.) It's just a different arrangement of the same atoms. It's like making a Lego sculpture, then taking it apart and using the exact same Legos to make a completely different sculpture.
to speed up a chemical reaction .. we use a catalyst
its a chemical reaction because you cannot undo it