Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

[imak_83]

Asslam o Alaikum

Ab mere taraf se aik Question.....

Taizaab jo her cheez ko jala daita hai.............to apnay ghar ko kue nahi jalaata ( jis mai rahta hai us ko)

Kia wo itna samajdar hai k us ko pata hai ager is ko jala doonga to phir rahu ga kahan?????


thAnks,

Muhammad Imak

[AbgeenA]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

sorry mujhe nahi pata:blush:

[Nisa*]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

Asslam o Alaikum

Ab mere taraf se aik Question.....

Taizaab jo her cheez ko jala daita hai.............to apnay ghar ko kue nahi jalaata ( jis mai rahta hai us ko)

Kia wo itna samajdar hai k us ko pata hai ager is ko jala doonga to phir rahu ga kahan?????


thAnks,

Muhammad Imak

Ajnabi :tauba yeh tho acid hi behtar bata sakta hay:khi: wesy sawal hay bahut acha sochney ki baat tho hey:cc:
wasalaam...

[imak_83]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

Sochnay ke baat to hai lakin sochna mat......kue boj daalna baicharay per
Btw - sochnay wali device to hai na:khi:

[Nisa*]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

Sochnay ke baat to hai lakin sochna mat......kue boj daalna baicharay per
Btw - sochnay wali device to hai na:khi:

achaa:hathora

[imak_83]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

ye apni khud he pitaii kar rahi ho .... kue bai

[D@y W@lk3r]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

Asslam o Alaikum

Ab mere taraf se aik Question.....

Taizaab jo her cheez ko jala daita hai.............to apnay ghar ko kue nahi jalaata ( jis mai rahta hai us ko)

Kia wo itna samajdar hai k us ko pata hai ager is ko jala doonga to phir rahu ga kahan?????


thAnks,

Muhammad Imak

lol kiya chemistry nahi pari.


Forms of sulfuric acid
Although nearly 100% sulfuric acid can be made, this loses SO3 at the boiling point to produce 98.3% acid. The 98% grade is more stable in storage, and is the usual form of what is described as concentrated sulfuric acid. Other concentrations are used for different purposes. Some common concentrations are

• 10%, dilute sulfuric acid for laboratory use,
• 33.5%, battery acid (used in lead-acid batteries),
• 62.18%, chamber or fertilizer acid,
• 77.67%, tower or Glover acid,
• 98%, concentrated acid.

Different purities are also available. Technical grade H2SO4 is impure and often colored, but is suitable for making fertilizer. Pure grades such as US Pharmacopoeia (USP) grade are used for making pharmaceuticals and dyestuffs.
When high concentrations of SO3(g) are added to sulfuric acid, H2S2O7, called pyrosulfuric acid, fuming sulfuric acid or oleum or, less commonly, Nordhausen acid

Polarity and conductivity

Anhydrous H2SO4 is a very polar liquid, with a dielectric constant of around 100. This is due to the fact that it can dissociate by protonating itself, a process known as autoprotolysis,[2] which occurs to a high degree, more than 10 billion times the level seen in water:
2 H2SO4 ⇌ H3SO4+ + HSO4− This allows protons to be highly mobile in H2SO4. It also makes sulfuric acid an excellent solvent for many reactions. In fact, the equilibrium is more complex than shown above. 100% H2SO4 contains the following species at equilibrium (figures shown as mol per kg solvent): HSO4− (15.0), H3SO4+ (11.3), H3O+ (8.0), HS2O7− (4.4), H2S2O7 (3.6), H2O (0.1).

Sulfuric acid is produced from sulfur, oxygen and water via the contact process.
In the first step, sulfur is burned to produce sulfur dioxide.
(1) S(s) + O2(g) → SO2(g) This is then oxidised to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst.
(2) 2 SO2 + O2(g) → 2 SO3(g) (in presence of V2O5) Finally the sulfur trioxide is treated with water (usually as 97-98% H2SO4 containing 2-3% water) to produce 98-99% sulfuric acid.
(3) SO3(g) + H2O(l) → H2SO4(l) Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Mists are formed instead of a liquid. Alternatively, SO3 can be absorbed into H2SO4 to produce oleum (H2S2O7), which may then be mixed with water to form sulfuric acid.
(3) H2SO4(l) + SO3 → H2S2O7(l) Oleum is reacted with water to form concentrated H2SO4.
(4) H2S2O7(l) + H2O(l) → 2 H2SO4(l) In 1993, American production of sulfuric acid amounted to 36.4 million tonnes. World production in 2001 was 165 million tonnes.

Sulfur-iodine cycle
The sulfur-iodine cycle is a series of thermo-chemical processes used to obtain hydrogen. It consists of three chemical reactions whose net reactant is water and whose net products are hydrogen and oxygen.
The sulfur and iodine compounds are recovered and reused, hence the consideration of the process as a cycle. This process is endothermic and must occur at high temperatures, so energy in the form of heat has to be supplied.
The sulfur-iodine cycle has been proposed as a way to supply hydrogen for a hydrogen-based economy. It does not require hydrocarbons like current methods of steam reforming.
The sulfur-iodine cycle is currently being researched as a feasible method of obtaining hydrogen, but the concentrated, corrosive acid at high temperatures poses currently insurmountable safety hazards if the process were built on large-scale.

Although sulfuric acid is non-flammable, contact with metals in the event of a spillage can lead to the liberation of hydrogen gas. The dispersal of acid aerosols and gaseous sulfur dioxide is an additional hazard of fires involving sulfuric acid. Water should not be used as the extinguishing agent because of the risk of further dispersal of aerosols: carbon dioxide is preferred where possible.
Sulfuric acid is not considered toxic besides its obvious corrosive hazard, and the main occupational risks are skin contact leading to burns (see above) and the inhalation of aerosols. Exposure to aerosols at high concentrations leads to immediate and severe irritation of the eyes, respiratory tract and mucous membranes: this ceases rapidly after exposure, although there is a risk of subsequent pulmonary edema if tissue damage has been more severe. At lower concentrations, the most commonly reported symptom of chronic exposure to sulfuric acid aerosols is erosion of the teeth, found in virtually all studies: indications of possible chronic damage to the respiratory tract are inconclusive as of 1997. In the United States, the permissible exposure limit (PEL) for sulfuric acid is fixed at 1 mg/m3: limits in other countries are similar. Interestingly there have been reports of sulfuric acid ingestion leading to vitamin B12 deficiency with subacute combined degeneration. The spinal cord is most often affected in such cases, but the optic nerves may show demyelination, loss of axons and gliosis.

[Nisa*]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

ye apni khud he pitaii kar rahi ho .... kue bai

hum nahi hay aap ghor sey dekay :lpop:

[sccorpion81]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

lol kiya chemistry nahi pari.


Forms of sulfuric acid
Although nearly 100% sulfuric acid can be made, this loses SO3 at the boiling point to produce 98.3% acid. The 98% grade is more stable in storage, and is the usual form of what is described as concentrated sulfuric acid. Other concentrations are used for different purposes. Some common concentrations are

• 10%, dilute sulfuric acid for laboratory use,
• 33.5%, battery acid (used in lead-acid batteries),
• 62.18%, chamber or fertilizer acid,
• 77.67%, tower or Glover acid,
• 98%, concentrated acid.

Different purities are also available. Technical grade H2SO4 is impure and often colored, but is suitable for making fertilizer. Pure grades such as US Pharmacopoeia (USP) grade are used for making pharmaceuticals and dyestuffs.
When high concentrations of SO3(g) are added to sulfuric acid, H2S2O7, called pyrosulfuric acid, fuming sulfuric acid or oleum or, less commonly, Nordhausen acid

Polarity and conductivity

Anhydrous H2SO4 is a very polar liquid, with a dielectric constant of around 100. This is due to the fact that it can dissociate by protonating itself, a process known as autoprotolysis,[2] which occurs to a high degree, more than 10 billion times the level seen in water:
2 H2SO4 ⇌ H3SO4+ + HSO4− This allows protons to be highly mobile in H2SO4. It also makes sulfuric acid an excellent solvent for many reactions. In fact, the equilibrium is more complex than shown above. 100% H2SO4 contains the following species at equilibrium (figures shown as mol per kg solvent): HSO4− (15.0), H3SO4+ (11.3), H3O+ (8.0), HS2O7− (4.4), H2S2O7 (3.6), H2O (0.1).

Sulfuric acid is produced from sulfur, oxygen and water via the contact process.
In the first step, sulfur is burned to produce sulfur dioxide.
(1) S(s) + O2(g) → SO2(g) This is then oxidised to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst.
(2) 2 SO2 + O2(g) → 2 SO3(g) (in presence of V2O5) Finally the sulfur trioxide is treated with water (usually as 97-98% H2SO4 containing 2-3% water) to produce 98-99% sulfuric acid.
(3) SO3(g) + H2O(l) → H2SO4(l) Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Mists are formed instead of a liquid. Alternatively, SO3 can be absorbed into H2SO4 to produce oleum (H2S2O7), which may then be mixed with water to form sulfuric acid.
(3) H2SO4(l) + SO3 → H2S2O7(l) Oleum is reacted with water to form concentrated H2SO4.
(4) H2S2O7(l) + H2O(l) → 2 H2SO4(l) In 1993, American production of sulfuric acid amounted to 36.4 million tonnes. World production in 2001 was 165 million tonnes.

Sulfur-iodine cycle
The sulfur-iodine cycle is a series of thermo-chemical processes used to obtain hydrogen. It consists of three chemical reactions whose net reactant is water and whose net products are hydrogen and oxygen.
The sulfur and iodine compounds are recovered and reused, hence the consideration of the process as a cycle. This process is endothermic and must occur at high temperatures, so energy in the form of heat has to be supplied.
The sulfur-iodine cycle has been proposed as a way to supply hydrogen for a hydrogen-based economy. It does not require hydrocarbons like current methods of steam reforming.
The sulfur-iodine cycle is currently being researched as a feasible method of obtaining hydrogen, but the concentrated, corrosive acid at high temperatures poses currently insurmountable safety hazards if the process were built on large-scale.

Although sulfuric acid is non-flammable, contact with metals in the event of a spillage can lead to the liberation of hydrogen gas. The dispersal of acid aerosols and gaseous sulfur dioxide is an additional hazard of fires involving sulfuric acid. Water should not be used as the extinguishing agent because of the risk of further dispersal of aerosols: carbon dioxide is preferred where possible.
Sulfuric acid is not considered toxic besides its obvious corrosive hazard, and the main occupational risks are skin contact leading to burns (see above) and the inhalation of aerosols. Exposure to aerosols at high concentrations leads to immediate and severe irritation of the eyes, respiratory tract and mucous membranes: this ceases rapidly after exposure, although there is a risk of subsequent pulmonary edema if tissue damage has been more severe. At lower concentrations, the most commonly reported symptom of chronic exposure to sulfuric acid aerosols is erosion of the teeth, found in virtually all studies: indications of possible chronic damage to the respiratory tract are inconclusive as of 1997. In the United States, the permissible exposure limit (PEL) for sulfuric acid is fixed at 1 mg/m3: limits in other countries are similar. Interestingly there have been reports of sulfuric acid ingestion leading to vitamin B12 deficiency with subacute combined degeneration. The spinal cord is most often affected in such cases, but the optic nerves may show demyelination, loss of axons and gliosis.

:tauba yeh kon perhay ga???:embarasse
mere khyal main ummid sara perh lay gee:D

[D@y W@lk3r]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

:tauba yeh kon perhay ga???:embarasse
mere khyal main ummid sara perh lay gee:D

ji to phir app idher kiya kar rahay hain........... Ummid to hain Mashallha zaheen bachi...

[ChaMpioN PaKiStaNi]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

lol kiya chemistry nahi pari.


Forms of sulfuric acid
Although nearly 100% sulfuric acid can be made, this loses SO3 at the boiling point to produce 98.3% acid. The 98% grade is more stable in storage, and is the usual form of what is described as concentrated sulfuric acid. Other concentrations are used for different purposes. Some common concentrations are

• 10%, dilute sulfuric acid for laboratory use,
• 33.5%, battery acid (used in lead-acid batteries),
• 62.18%, chamber or fertilizer acid,
• 77.67%, tower or Glover acid,
• 98%, concentrated acid.

Different purities are also available. Technical grade H2SO4 is impure and often colored, but is suitable for making fertilizer. Pure grades such as US Pharmacopoeia (USP) grade are used for making pharmaceuticals and dyestuffs.
When high concentrations of SO3(g) are added to sulfuric acid, H2S2O7, called pyrosulfuric acid, fuming sulfuric acid or oleum or, less commonly, Nordhausen acid

Polarity and conductivity

Anhydrous H2SO4 is a very polar liquid, with a dielectric constant of around 100. This is due to the fact that it can dissociate by protonating itself, a process known as autoprotolysis,[2] which occurs to a high degree, more than 10 billion times the level seen in water:
2 H2SO4 ⇌ H3SO4+ + HSO4− This allows protons to be highly mobile in H2SO4. It also makes sulfuric acid an excellent solvent for many reactions. In fact, the equilibrium is more complex than shown above. 100% H2SO4 contains the following species at equilibrium (figures shown as mol per kg solvent): HSO4− (15.0), H3SO4+ (11.3), H3O+ (8.0), HS2O7− (4.4), H2S2O7 (3.6), H2O (0.1).

Sulfuric acid is produced from sulfur, oxygen and water via the contact process.
In the first step, sulfur is burned to produce sulfur dioxide.
(1) S(s) + O2(g) → SO2(g) This is then oxidised to sulfur trioxide using oxygen in the presence of a vanadium(V) oxide catalyst.
(2) 2 SO2 + O2(g) → 2 SO3(g) (in presence of V2O5) Finally the sulfur trioxide is treated with water (usually as 97-98% H2SO4 containing 2-3% water) to produce 98-99% sulfuric acid.
(3) SO3(g) + H2O(l) → H2SO4(l) Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Mists are formed instead of a liquid. Alternatively, SO3 can be absorbed into H2SO4 to produce oleum (H2S2O7), which may then be mixed with water to form sulfuric acid.
(3) H2SO4(l) + SO3 → H2S2O7(l) Oleum is reacted with water to form concentrated H2SO4.
(4) H2S2O7(l) + H2O(l) → 2 H2SO4(l) In 1993, American production of sulfuric acid amounted to 36.4 million tonnes. World production in 2001 was 165 million tonnes.

Sulfur-iodine cycle
The sulfur-iodine cycle is a series of thermo-chemical processes used to obtain hydrogen. It consists of three chemical reactions whose net reactant is water and whose net products are hydrogen and oxygen.
The sulfur and iodine compounds are recovered and reused, hence the consideration of the process as a cycle. This process is endothermic and must occur at high temperatures, so energy in the form of heat has to be supplied.
The sulfur-iodine cycle has been proposed as a way to supply hydrogen for a hydrogen-based economy. It does not require hydrocarbons like current methods of steam reforming.
The sulfur-iodine cycle is currently being researched as a feasible method of obtaining hydrogen, but the concentrated, corrosive acid at high temperatures poses currently insurmountable safety hazards if the process were built on large-scale.

Although sulfuric acid is non-flammable, contact with metals in the event of a spillage can lead to the liberation of hydrogen gas. The dispersal of acid aerosols and gaseous sulfur dioxide is an additional hazard of fires involving sulfuric acid. Water should not be used as the extinguishing agent because of the risk of further dispersal of aerosols: carbon dioxide is preferred where possible.
Sulfuric acid is not considered toxic besides its obvious corrosive hazard, and the main occupational risks are skin contact leading to burns (see above) and the inhalation of aerosols. Exposure to aerosols at high concentrations leads to immediate and severe irritation of the eyes, respiratory tract and mucous membranes: this ceases rapidly after exposure, although there is a risk of subsequent pulmonary edema if tissue damage has been more severe. At lower concentrations, the most commonly reported symptom of chronic exposure to sulfuric acid aerosols is erosion of the teeth, found in virtually all studies: indications of possible chronic damage to the respiratory tract are inconclusive as of 1997. In the United States, the permissible exposure limit (PEL) for sulfuric acid is fixed at 1 mg/m3: limits in other countries are similar. Interestingly there have been reports of sulfuric acid ingestion leading to vitamin B12 deficiency with subacute combined degeneration. The spinal cord is most often affected in such cases, but the optic nerves may show demyelination, loss of axons and gliosis.

:thmbup: yes hum ne read kiya tha FSC main

[ummid]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

:tauba yeh kon perhay ga???:embarasse
mere khyal main ummid sara perh lay gee:D

:slap:

ji to phir app idher kiya kar rahay hain........... Ummid to hain Mashallha zaheen bachi...

:blush: thankooo... per bhai hum ne nahi parha...:embarasse

[D@y W@lk3r]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

:slap:



:blush: thankooo... per bhai hum ne nahi parha...:embarasse

to phir app nay kiya parha.

[ummid]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

to phir app nay kiya parha.

woh na hum itna sara likha hai tu hum KUL parhleinge...:embarasse
aap gussa na kijye...

[Abdul Qudoos]

Re: Taizaab (Acid) Kue nahi Jalata apny Ghar ko????

sirf aik hi gawab kion kay woh Gadar Nahi