anonymous
  • anonymous
Contact Process Questions for a project. Okay, I have answered some of these, but need help with the rest. Just give me a moment to post them all separately (the word count is too high for this entry).
Chemistry
  • Stacey Warren - Expert brainly.com
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chestercat
  • chestercat
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
anonymous
  • anonymous
Q: Describe the process you researched, including its uses in various industrial or health fields. A: The contact process is used to create sulfuric acid. Sulfur dioxide and oxygen pass over a hot catalyst and unite to create sulfur trioxide. It then reacts with water to create sulfuric acid. Q: Who developed or discovered this process? When? What country was he or she from? (Provide this information if you can find it.) A: Although the first observation of the contact process was by Edmund Davy in 1817, it was first patented in 1831 by Peregrine Phillips. Phillips was from Bristol, England. Q: Provide a short paragraph providing some historical background. Why is, or was, this an important chemical process? A: I can't really find anything, then again I'm super tired, only got 3 hours of sleep last night, so I'm dragging and just need help on this part. Maybe give me like 4-5 sentences? Q: Write a balanced chemical equation for this reaction, including the energy term. Is it an endothermic or exothermic reaction? A: I need an answer for this, I don't even understand what it's trying to ask. I'm assuming it's Endothermic, but I am probably remembering wrong. I still need help on the equation part. Q: Use Le Châtelier’s principle to explain the conditions that favor the forward reaction. A: Ummm? Help please? Q: Under what temperature, pressure, and other conditions is this reaction typically carried out? How does this relate to part of your answer for Question 3? A: I know it's under high temperatures, but I don't know the rest of it. Q: What safety, cost, or other considerations prevent most industrial applications from using the most ideal conditions for high yield of the product? A: Umm, I'm sure it costs a lot, I'm not sure what's safe or unsafe about it. So I need help on this. Q: What catalyst, if any, is used for this reaction? A: Heated Platinum was the catalyst used for this process.
anonymous
  • anonymous
Thank you to anyone who helps on this, it would mean a lot. I just need the answers short so I can stretch them out and create a good essay. Wording and grammar doesn't mean much because I'll change it to my own, I just need it to make sense.
.Sam.
  • .Sam.
For the reactions Reaction is exothermic \[S+O2->SO2\] \[2SO2+O2->2SO3\] \[SO3+2H2O \leftarrow \rightarrow H2SO4\] Hot sulphur trioxide passes through the heat exchanger and is dissolved in concentrated H2SO4 in the absorption tower to form oleum: H2SO4(l) + SO3(g) → H2S2O7(l) Note that directly dissolving SO3 in water is impractical due to the highly exothermic nature of the reaction. Acidic vapor or mists are formed instead of a liquid. Oleum is reacted with water to form concentrated H2SO4. The average percentage yield of this reaction is around 30%. H2S2O7(l) + H2O(l) → 2 H2SO4(l)

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.Sam.
  • .Sam.
They normally use V2O5 for catalyst
anonymous
  • anonymous
Thank you so far (: I'm hoping I can get all caught up on my Chemistry tonight... I'm sooo tired -_-'
.Sam.
  • .Sam.
the overall reaction is \[2 SO2(g) + O2(g) ⇌ 2 SO3(g)\] its a 4 to 3 ratio Notice that there are 3 molecules on the left-hand side of the equation, but only 2 on the right. according to Le Chatelier's Principle, if you increase the pressure the system will respond by favouring the reaction which produces fewer molecules. That will cause the pressure to fall again. In order to get as much sulphur trioxide as possible in the equilibrium mixture, you need as high a pressure as possible. High pressures also increase the rate of the reaction. according to Le Chatelier's Principle, Increasing the concentration of oxygen in the mixture causes the position of equilibrium to shift towards the right. Since the oxygen comes from the air, this is a very cheap way of increasing the conversion of sulphur dioxide into sulphur trioxide. In order to get as much sulphur trioxide as possible in the equilibrium mixture, you need as low a temperature as possible. The forward reaction (the production of sulphur trioxide) is exothermic. According to Le Chatelier's Principle, this will be favoured if you lower the temperature.
Callisto
  • Callisto
Condition for Contact process: 450 degree Celsius, 1 atm V2O5 2SO2 + O2 ----------------> 2SO3 (g) <------------------ 450°C, 1atm That's what I've got from my book :|
Callisto
  • Callisto
To my knowledge, contact process is exothermic So, for the question; Use Le Châtelier’s principle to explain the conditions that favor the forward reaction. Since it's a exothermic reaction, according to the Le Châtelier’s principle, lower temperature favours the forward reaction, hence, giving a high percentage yield of SO3 To be simple: ↓T ->↑ percentage yield From the equation, Total no. of mole of gases on the left = 2+1 = 3 Total no. of mole of gases on the right = 2 <3 So, according to the Le Châtelier’s principle, lower pressure favours the forward reaction, which gives a higher percentage yield of SO3 To be simple: ↓pressure ->↑ percentage yield
anonymous
  • anonymous
Thank you for your answers(:

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