What are the products formed when nitrogen dioxide reacts with water?












3














I've seen two different equations for the reaction of nitrogen dioxide with water:



$$ce{2NO2 + H2O -> H+ + NO3- + HNO2}$$



and



$$ce{3NO2 + H2O -> 2H+ + 2NO3- + NO}$$



Are both of these correct to some degree, and is one more prominent over the other?






inorganic-chemistry redox







share|improve this question





























    3














    I've seen two different equations for the reaction of nitrogen dioxide with water:



    $$ce{2NO2 + H2O -> H+ + NO3- + HNO2}$$



    and



    $$ce{3NO2 + H2O -> 2H+ + 2NO3- + NO}$$



    Are both of these correct to some degree, and is one more prominent over the other?






    inorganic-chemistry redox







    share|improve this question



























      3












      3








      3







      I've seen two different equations for the reaction of nitrogen dioxide with water:



      $$ce{2NO2 + H2O -> H+ + NO3- + HNO2}$$



      and



      $$ce{3NO2 + H2O -> 2H+ + 2NO3- + NO}$$



      Are both of these correct to some degree, and is one more prominent over the other?






      inorganic-chemistry redox







      share|improve this question















      I've seen two different equations for the reaction of nitrogen dioxide with water:



      $$ce{2NO2 + H2O -> H+ + NO3- + HNO2}$$



      and



      $$ce{3NO2 + H2O -> 2H+ + 2NO3- + NO}$$



      Are both of these correct to some degree, and is one more prominent over the other?






      inorganic-chemistry redox




      inorganic-chemistry redox






      share|improve this question















      share|improve this question













      share|improve this question




      share|improve this question








      edited 10 mins ago









      orthocresol♦

      38k7111229




      38k7111229










      asked 5 hours ago









      chemN00b

      224




      224






















          2 Answers
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          2














          Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.



          When nitrogen dioxide($ce{NO2}$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ce{HNO3)}$ and nitrous acid(HNO2). $$ce{2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)}$$
          i.e.$$ce{2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)}$$



          However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ce{NO}$ and $ce{HNO3}$:
          $$ce{3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)}$$



          Your second reaction equation is obtained by adding these two reaction together.



          Reference:




          1. Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.


          Note:



          I wrote the $ce{H+}$ ions as $ce{H3O+}$, so there is an extra water molecule on the left side of the equation, in each case.






          share|improve this answer































            1














            Both can take place, but nitrous acid is unstable. In warm or concentrated solutions, the nitrous acid will disproportionate, forming nitric oxide and more nitric acid. So the nitrous acid is essentially only a temporary intermediate.






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              2 Answers
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              2 Answers
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              active

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              active

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              2














              Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.



              When nitrogen dioxide($ce{NO2}$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ce{HNO3)}$ and nitrous acid(HNO2). $$ce{2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)}$$
              i.e.$$ce{2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)}$$



              However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ce{NO}$ and $ce{HNO3}$:
              $$ce{3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)}$$



              Your second reaction equation is obtained by adding these two reaction together.



              Reference:




              1. Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.


              Note:



              I wrote the $ce{H+}$ ions as $ce{H3O+}$, so there is an extra water molecule on the left side of the equation, in each case.






              share|improve this answer




























                2














                Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.



                When nitrogen dioxide($ce{NO2}$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ce{HNO3)}$ and nitrous acid(HNO2). $$ce{2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)}$$
                i.e.$$ce{2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)}$$



                However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ce{NO}$ and $ce{HNO3}$:
                $$ce{3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)}$$



                Your second reaction equation is obtained by adding these two reaction together.



                Reference:




                1. Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.


                Note:



                I wrote the $ce{H+}$ ions as $ce{H3O+}$, so there is an extra water molecule on the left side of the equation, in each case.






                share|improve this answer


























                  2












                  2








                  2






                  Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.



                  When nitrogen dioxide($ce{NO2}$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ce{HNO3)}$ and nitrous acid(HNO2). $$ce{2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)}$$
                  i.e.$$ce{2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)}$$



                  However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ce{NO}$ and $ce{HNO3}$:
                  $$ce{3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)}$$



                  Your second reaction equation is obtained by adding these two reaction together.



                  Reference:




                  1. Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.


                  Note:



                  I wrote the $ce{H+}$ ions as $ce{H3O+}$, so there is an extra water molecule on the left side of the equation, in each case.






                  share|improve this answer














                  Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.



                  When nitrogen dioxide($ce{NO2}$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ce{HNO3)}$ and nitrous acid(HNO2). $$ce{2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)}$$
                  i.e.$$ce{2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)}$$



                  However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ce{NO}$ and $ce{HNO3}$:
                  $$ce{3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)}$$



                  Your second reaction equation is obtained by adding these two reaction together.



                  Reference:




                  1. Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.


                  Note:



                  I wrote the $ce{H+}$ ions as $ce{H3O+}$, so there is an extra water molecule on the left side of the equation, in each case.







                  share|improve this answer














                  share|improve this answer



                  share|improve this answer








                  edited 9 mins ago









                  orthocresol♦

                  38k7111229




                  38k7111229










                  answered 2 hours ago









                  Shoubhik Raj Maiti

                  1,269529




                  1,269529























                      1














                      Both can take place, but nitrous acid is unstable. In warm or concentrated solutions, the nitrous acid will disproportionate, forming nitric oxide and more nitric acid. So the nitrous acid is essentially only a temporary intermediate.






                      share|improve this answer


























                        1














                        Both can take place, but nitrous acid is unstable. In warm or concentrated solutions, the nitrous acid will disproportionate, forming nitric oxide and more nitric acid. So the nitrous acid is essentially only a temporary intermediate.






                        share|improve this answer
























                          1












                          1








                          1






                          Both can take place, but nitrous acid is unstable. In warm or concentrated solutions, the nitrous acid will disproportionate, forming nitric oxide and more nitric acid. So the nitrous acid is essentially only a temporary intermediate.






                          share|improve this answer












                          Both can take place, but nitrous acid is unstable. In warm or concentrated solutions, the nitrous acid will disproportionate, forming nitric oxide and more nitric acid. So the nitrous acid is essentially only a temporary intermediate.







                          share|improve this answer












                          share|improve this answer



                          share|improve this answer










                          answered 2 hours ago









                          Oscar Lanzi

                          14.6k12546




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