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a) MgCl2(aq) + NaOH(aq) ---> Mg(OH)2(s) + NaCl (aqThe amount of AgNO3: 50.00 mL of 0.2000M AgNO3(aq)

The amount of CaCl2: 24.85.00 mL of 0.1012 M CaCl2(aq)
Mass of filter paper, m(f) = 2.032 g
Mass of filter paper + precipitate, m(f+p) = 3.178 g
Upon mixing of the two clear solutions of AgNO3 and CaCl2 a very fine white precipitate was immediately formed causing the reaction mixture to become milky.
It took approximately 25 minutes before the excess liquid was drained away during the filtration.
After one hour of air drying, the product was found to be a very fine powder.


CALCULATIONS AND RESULTS:
Reaction equation: 2 AgNO3(aq) + CaCl2(aq) > 2 AgCl(s) + Ca(NO3)2(aq)

Determination of the # of moles; n = cV


Pb(NO3)2 + 2 KI ==> PbI2¯ + 2 KNO3 (8.1) ... of a simple mixing of approximately equal volumes of KI and Pb(NO3)2 solutions.

alkali ----> salt + ammonia +water: NH4Cl(aq)+NaOH(aq) ->NaCl(aq)+NH3(g) ... NH4Cl(aq)+NaOH(aq) ->NaCl(aq)+NH3(g)+H2O(l) (or NH4+(aq)+OH-(aq) ->NH3(aq)+H2O(l)

Sulfur dioxide (also sulphur dioxide) is the chemical compound with the formula SO2. This important gas is the main product from the combustion of sulfur compounds and is of significant environmental concern. SO2 is often described as the "smell of burning sulfur" but is not responsible for the smell of rotten eggs.
SO2 is produced by volcanoes and in various industrial processes. Since coal and petroleum contain various amounts of sulfur compounds, their combustion generates sulfur dioxide. Further oxidation of SO2, usually in the presence of a catalyst such as NO2, forms H2SO4, and thus acid rain.[2]
Sulfur dioxide can be prepared by burning sulfur:
S8(s) + 8O2(g) → 8SO2(g)
The combustion of hydrogen sulfide and organosulfur compounds proceeds similarly.
2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)
The roasting of sulfide ores such as iron pyrites, sphalerite (zinc blende) and cinnabar (mercury sulfide) also emits SO2:
4FeS2(s) + 11O2(g) → 2Fe2O3(s) + 8SO2(g)
2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g)
HgS(s) + O2(g) → Hg(g) + SO2(g)
When anhydrous CaSO4 is heated with coke and sand in the manufacture of cement, CaSiO3, sulfur dioxide is a by-product.
2CaSO4(s) + 2SiO2(s) + C(s) → 2CaSiO3(s) + 2SO2(g) + CO2(g)
Action of hot concentrated sulfuric acid on copper turnings will produce sulfur dioxide.
Cu(s) + 2H2SO4(aq) → CuSO4(aq) + SO2(g) + 2H2O(l)



Sulfur dioxide blocks nerve signals from the pulmonary stretch receptors (PSR's) and abolishes the Hering-Breuer inflation reflex.
Prior to the development of freons, sulfur dioxide was used as a refrigerant in home refrigerators.
Sulfur dioxide is the anhydride of sulfurous acid, H2SO3.
SO2 is also a very important element in winery sanitation. Wineries and equipment must be kept very clean, and because bleach cannot be used in a winery, a mixture of SO2, water, and citric acid is commonly used to clean hoses, tanks, and other equipment to keep it clean and free of bacteria.





Biosphere II was created in 1991 to test the idea that scientists could build a sealed, self-2. Q: Biosphere II was created in 1991 to test the idea that scientists could build a sealed, self-sustaining ecosystem. The carbon dioxide levels in Biosphere II were lower than scientists had predicted. Scientists discovered that the carbon dioxide was reacting with calcium hydroxide, a basic compound in the concrete. dioxide levels in Biosphere II were lower than scientists had predicted. Scientists discovered that the carbon dioxide was reacting with calcium hydroxide, a basic compou

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