Magnesium n Manganese react with dil.HNO3 to evolve H2 gas.However, HNO3 (nitric acid) is a strong oxidizing agent. It oxidizes H2 to H2O & itself gets reduced to any of the Nitrogen oxides (N2O, NO, NO2). Hope it is informative!!!!
Neither Mg, nor Mn can reduce H+ of HNO3 to H2 because NO3- is a much stronger oxydizer. A redox reaction will happen always between the most powerful oxydizer (here NO3- and not H+) and the most powerful reducer (here, metals), because their delta Gibbs energy is much bigger. It's better to return to school. ;)
@@parvizallazov5194They can, but either it takes extra metal and or time, or it happens in two steps. The first is the nitric acid decomposes into water, oxygen, and nitrogen oxides, the second is the metal liberating hydrogen from the water.
Hello and thank you for the question. The reaction between magnesium and concentrated (70%) nitric acid is vigorous and should only be carried out following the appropriate precautions. The reaction is highly exothermic (you may with to do the thermochemistry behind it as part of your ISA) and produces a mixture of toxic gases (nitrogen oxides). Concentrated nitric acid is highly oxidising and magnesium is a strong reducing agent, which is part of the reason why this reaction is so vigorous. It is important to consider the concentration of the acid for the reaction, as at low concentrations a different reaction can take place, and the reaction can be more vigorous if using the more concentrated 'fuming' nitric acid. For the safety information behind the 70% nitric acid used in this video, please refer to the following link: www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=GB&language=en&productNumber=438073&brand=FLUKA&PageToGoToURL=http%3A%2F%2Fwww.sigmaaldrich.com%2Fcatalog%2Fproduct%2Ffluka%2F438073%3Flang%3Den In regards to the gases produced, it is mostly nitrogen dioxide (once again see the link below for safety info) along with nitric acid fumes due to the increased temperature. The rise in temperature can also cause the formation of many other nitrogen oxides, but in lesser quantities. www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=GB&language=en&productNumber=295582&brand=ALDRICH&PageToGoToURL=http%3A%2F%2Fwww.sigmaaldrich.com%2Fcatalog%2Fproduct%2Faldrich%2F295582%3Flang%3Den If you have any further questions then I am happy to help. Please remember to reference this if it is a part of your ISA.
thank you so much for replying ! what is "highly oxidsing " and in relation to context do you know how surface area in rate of reaction may be useful in industry ? i was going to use 1.5 mol is this too weak ?
Oxidising agents facilitate loss of electrons and since the nitrate anion has three oxygen atoms (highly electronegative, they will happily accept electrons from other species to from more stable structures). The nitrate anion is also quite stable as it has three resonance forms, and this is one explanation as to why nitric acid is such a strong acid. Having a strong acid means that there is lots of hydrogen ions in solution, which help to form the more stable products once the nitrate anion has accepted electrons from the metal. I am unfamiliar with the mechanism I'm afraid, but you could probably find it somewhere online. To have the oxidising effect, 1.5M is probably a little bit too weak (although I have never tried with that specific concentration) and you may end up with a classic acid-metal reaction rather than the formation of many nitrogen oxides. A short practical could be set up to determine if this is the case. Make sure you have direct supervision of your teacher/tutor (who has appropriate laboratory experience) when carrying out any reactions like this or when handling nitric acid as there are many hidden dangers (one of which includes latex gloves catching alight when exposed to concentrated nitric). Increasing the surface area will increase the rate of reaction. If I had used powdered magnesium in this video it would have been much more vigorous (and dangerous). I have relatively little industrial experience, but it would be a balance between safety and speed when determining the surface area of a solid reactant to use. As far as I am aware, the reactions used in this video are not typical reactions bulked-up in industry.
not that s best way to reach kno3 for me if i can buy any nitrate salt i can produce from other salt but i cant so i must get nitrate from nitric acid and its very pure just must be calculated the mole of reaction
Impressive but very scary. I made 10 percent Nitric acid with 20 percent rest being HCl it was more reactive to zinc powder than copper powder. For Antimony it was a very slow process that is always a tricky metal to oxidize.
+Blue Vortex Thank you for pointing this out. I did not realise that there was a mistake within the video, and it is quite obvious from the footage of the reaction that nitrogen dioxide gas (orange-brown) is produced as a result of the reactions. I shall re-edit the video soon.
So awesome to see actual reactions instead of just equations!!!!
So that's how to make Fanta
McC1oudv2 is it???
you didnt get the joke?
😂😂😂
Fanta(stic)😂😂😂
It’s all about the fanta…sy yeeeeaaaah 🎶
Magnesium n Manganese react with dil.HNO3 to evolve H2 gas.However, HNO3 (nitric acid) is a strong oxidizing agent. It oxidizes H2 to H2O & itself gets reduced to any of the Nitrogen oxides (N2O, NO, NO2).
Hope it is informative!!!!
Yes thank you! I was trying to understand this concept😊
Neither Mg, nor Mn can reduce H+ of HNO3 to H2 because NO3- is a much stronger oxydizer. A redox reaction will happen always between the most powerful oxydizer (here NO3- and not H+) and the most powerful reducer (here, metals), because their delta Gibbs energy is much bigger. It's better to return to school. ;)
Remove 3 liked from the video, during my class it had 666 likes
@@parvizallazov5194 Better to return to the books*
Dumbass
@@parvizallazov5194They can, but either it takes extra metal and or time, or it happens in two steps. The first is the nitric acid decomposes into water, oxygen, and nitrogen oxides, the second is the metal liberating hydrogen from the water.
Guess what, i just witnessed that, but on a scale the size of a city a WHOLE CITY. Pray for lebanon 🙏 🇱🇧
Thank u it helped me in preparing for my science exam! :)
Hi sir,can I use this video in my UA-cam educational channel..IAM from Kerala,India.
They used it for our school too, in Galați, Romania
Can you react galinstan with nitric acid and then when the reaction is done add aluminum foil?
excellent camera work
What are the products formed in the reaction of nitric acid with zinc (both dilute and concentrated)? And it's very nice thank you!
according to theory it should be zinc nitrate and hydrogen
@@irwanahmed001 ohh tq... Btw I don't understand the ques asked by me 🙄
@@irwanahmed001 nitric acid is strong oxidising agent so it oxidises the hydrogen to water
Thank you very much for this video . Can you tell me please wich metal can i use in cementation of gold . ?
it,s looking so good. 👌👌👌
hi im doing my isa in chemistry , what risks are there with nitric acid and magnesium ,eg any gases or heat produced ? thanks
Hello and thank you for the question.
The reaction between magnesium and concentrated (70%) nitric acid is vigorous and should only be carried out following the appropriate precautions. The reaction is highly exothermic (you may with to do the thermochemistry behind it as part of your ISA) and produces a mixture of toxic gases (nitrogen oxides). Concentrated nitric acid is highly oxidising and magnesium is a strong reducing agent, which is part of the reason why this reaction is so vigorous.
It is important to consider the concentration of the acid for the reaction, as at low concentrations a different reaction can take place, and the reaction can be more vigorous if using the more concentrated 'fuming' nitric acid.
For the safety information behind the 70% nitric acid used in this video, please refer to the following link: www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=GB&language=en&productNumber=438073&brand=FLUKA&PageToGoToURL=http%3A%2F%2Fwww.sigmaaldrich.com%2Fcatalog%2Fproduct%2Ffluka%2F438073%3Flang%3Den
In regards to the gases produced, it is mostly nitrogen dioxide (once again see the link below for safety info) along with nitric acid fumes due to the increased temperature. The rise in temperature can also cause the formation of many other nitrogen oxides, but in lesser quantities.
www.sigmaaldrich.com/MSDS/MSDS/DisplayMSDSPage.do?country=GB&language=en&productNumber=295582&brand=ALDRICH&PageToGoToURL=http%3A%2F%2Fwww.sigmaaldrich.com%2Fcatalog%2Fproduct%2Faldrich%2F295582%3Flang%3Den
If you have any further questions then I am happy to help. Please remember to reference this if it is a part of your ISA.
thank you so much for replying ! what is "highly oxidsing " and in relation to context do you know how surface area in rate of reaction may be useful in industry ? i was going to use 1.5 mol is this too weak ?
Oxidising agents facilitate loss of electrons and since the nitrate anion has three oxygen atoms (highly electronegative, they will happily accept electrons from other species to from more stable structures).
The nitrate anion is also quite stable as it has three resonance forms, and this is one explanation as to why nitric acid is such a strong acid. Having a strong acid means that there is lots of hydrogen ions in solution, which help to form the more stable products once the nitrate anion has accepted electrons from the metal. I am unfamiliar with the mechanism I'm afraid, but you could probably find it somewhere online.
To have the oxidising effect, 1.5M is probably a little bit too weak (although I have never tried with that specific concentration) and you may end up with a classic acid-metal reaction rather than the formation of many nitrogen oxides. A short practical could be set up to determine if this is the case. Make sure you have direct supervision of your teacher/tutor (who has appropriate laboratory experience) when carrying out any reactions like this or when handling nitric acid as there are many hidden dangers (one of which includes latex gloves catching alight when exposed to concentrated nitric).
Increasing the surface area will increase the rate of reaction. If I had used powdered magnesium in this video it would have been much more vigorous (and dangerous). I have relatively little industrial experience, but it would be a balance between safety and speed when determining the surface area of a solid reactant to use. As far as I am aware, the reactions used in this video are not typical reactions bulked-up in industry.
Thanks a lot Sir ☺️..
1. Cu + 4HNO³ = Cu(NO³)² + 2NO² + 2H²O
2. Zn + 4HNO³ = Zn(NO³)² + 2NO² + 2H²O
3. Mg + 4HNO³ = Mg(NO³)² + 2NO² + 2H²O
Can u tell why lead dont give NO2 gas
ooh now it looks nice dude
Cool
If im working with large quantities of nitri acid, what can i do with the fumes beside burning them?
stop working with them XD
is that a lawnmower?
this is so coool
How much was the concentration of the nitric acid?
Sorry for the delay. It was 70% W/V (approx 15 M)
I tried using 1M of hno3
What will be the product of the reaction
1M of nitric acid with zinc and I got a dark green liquid..what could that be
pls can you show how to make potassium nitrate from nitric acid and potassium hidroxyde
Hmm, that looks ominous. It would actually be quite impractible to produce potassium nitrate of any purity in this way!
not that s best way to reach kno3 for me if i can buy any nitrate salt i can produce from other salt but i cant so i must get nitrate from nitric acid and its very pure just must be calculated the mole of reaction
Impressive but very scary. I made 10 percent Nitric acid with 20 percent rest being HCl it was more reactive to zinc powder than copper powder. For Antimony it was a very slow process that is always a tricky metal to oxidize.
nitric and hydrocloring acids as far as I remember can form NOCl (at least with concentrated acids) which is more powerful oxidizer than nitrate
your equations are all incorrect,Copper never makes hydrogen with ANY acid as its below Hydrogen the gas observed in all cases is Nitrogen Dioxide.
+Blue Vortex Thank you for pointing this out. I did not realise that there was a mistake within the video, and it is quite obvious from the footage of the reaction that nitrogen dioxide gas (orange-brown) is produced as a result of the reactions.
I shall re-edit the video soon.
My teacher provide this video to me
Ues full
Anyone in 2021
That orange gas is bad juju
Coper and Nitric acid = Copernicus
is it dil. or conc.
Arjit Gupta Thank you for your question! This video uses concentrated nitric acid.
Alex thanks and pls upload more i love chemistry