Question

Contact Process: What safety, cost, or other considerations prevent most industrial applications from using the most ideal conditions for high yield of the product?
Provide a short paragraph providing some historical background. Why is, or was, this an important chemical process?
I just need some help, please.

Answer 1

I have three websites and a web document open on the Contact process, reading about it, I just am having a difficult time figuring out these two questions. If I get the answers then I can do my paper, these are just guideline questions for my research paper.
I'd assume the cost for everything is really high which would cause the process to not be used as often? I'm having a little trouble on this., /:

Answer 2

quite a general question. if u cud be more specific, it might help.

Answer 3

Um those are as specific as it gets, bud.
The questions are about the Contact Process. What conditions and things could cause less ideal conditions for the process?
Why is or was the contact process important?
I just can't find much on these two. So far, anyway.

Answer 4

oh oops Contact Process

Answer 5

haha yeah

Answer 6

lol lemme see

Answer 7

Alright, thanks xD

Answer 8

I'm using these sites: http://www.chemguide.co.uk/physical/equilibria/contact.html
http://www.aiche-cf.org/Clearwater/2008/Paper2/8.2.7.pdf
http://www.britannica.com/EBchecked/topic/134642/contact-process
so yup xP

Answer 9

i think i got some idea. you there?

Answer 10

i think u r gone, anyways..

Importance: This process was patented in 1831by the British vinegar merchant Peregrine Phillips. In addition to being a far more economical process for producing concentrated sulphuric acid than the previous lead chamber process, the contact process also produces sulphur trioxide and oleum.

Answer 11

What considerations prevent most industrial applications from using the most ideal conditions for high yield of the product?

One of the equation in the process is:

Sulphur dioxide and oxygen then react as follows:

2 SO2(g) + O2(g) ⇌ 2 SO3(g) : ΔH = −197 kJ mol−1

According to the Le Chatelier's principle, a lower temperature should be used to shift the chemical equilibrium towards the right, hence increasing the percentage yield.

However too low of a temperature will lower the formation rate to an uneconomical level.

Hence to increase the reaction rate, high temperatures (450 °C), medium pressures (1-2 atm), and vanadium(V) oxide (V2O5) are used to ensure a 96% conversion.

~Trade off, basically~

Answer 12

hope it helps :)

Answer 13

Thanks(:

Answer 14

-wikipedia- can be gud place to search sometimes :)

Answer 15

It's not always accurate, though. Not supposed to use it for school.

Answer 16

lol yea...thats there..but u can gain some rough idea..

Answer 17

Yeah anything is better than nothing.
I just need to pass this class <.<

Answer 18

lol u will..c ya...bbye..