What are the products formed when nitrogen dioxide reacts with water?
Clash Royale CLAN TAG#URR8PPP
I've seen two different equations for the reaction of nitrogen dioxide with water:
$$ce2NO2 + H2O -> H+ + NO3- + HNO2$$
and
$$ce3NO2 + H2O -> 2H+ + 2NO3- + NO$$
Are both of these correct to some degree, and is one more prominent over the other?
inorganic-chemistry redox
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
add a comment |
I've seen two different equations for the reaction of nitrogen dioxide with water:
$$ce2NO2 + H2O -> H+ + NO3- + HNO2$$
and
$$ce3NO2 + H2O -> 2H+ + 2NO3- + NO$$
Are both of these correct to some degree, and is one more prominent over the other?
inorganic-chemistry redox
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
add a comment |
I've seen two different equations for the reaction of nitrogen dioxide with water:
$$ce2NO2 + H2O -> H+ + NO3- + HNO2$$
and
$$ce3NO2 + H2O -> 2H+ + 2NO3- + NO$$
Are both of these correct to some degree, and is one more prominent over the other?
inorganic-chemistry redox
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
I've seen two different equations for the reaction of nitrogen dioxide with water:
$$ce2NO2 + H2O -> H+ + NO3- + HNO2$$
and
$$ce3NO2 + H2O -> 2H+ + 2NO3- + NO$$
Are both of these correct to some degree, and is one more prominent over the other?
inorganic-chemistry redox
inorganic-chemistry redox
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
edited Dec 28 '18 at 23:41
orthocresol♦
38.4k7112233
38.4k7112233
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
asked Dec 28 '18 at 18:44
chemN00bchemN00b
519
519
add a comment |
add a comment |
2 Answers
2
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Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.
When nitrogen dioxide($ceNO2$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ceHNO3)$ and nitrous acid(HNO2). $$ce2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)$$
i.e.$$ce2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)$$
However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ceNO$ and $ceHNO3$:
$$ce3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)$$
Your second reaction equation is obtained by adding these two reaction together.
Reference:
- Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.
Note:
I wrote the $ceH+$ ions as $ceH3O+$, so there is an extra water molecule on the left side of the equation, in each case.
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
add a comment |
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.
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
add a comment |
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2 Answers
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2 Answers
2
active
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active
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active
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Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.
When nitrogen dioxide($ceNO2$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ceHNO3)$ and nitrous acid(HNO2). $$ce2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)$$
i.e.$$ce2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)$$
However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ceNO$ and $ceHNO3$:
$$ce3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)$$
Your second reaction equation is obtained by adding these two reaction together.
Reference:
- Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.
Note:
I wrote the $ceH+$ ions as $ceH3O+$, so there is an extra water molecule on the left side of the equation, in each case.
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
add a comment |
Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.
When nitrogen dioxide($ceNO2$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ceHNO3)$ and nitrous acid(HNO2). $$ce2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)$$
i.e.$$ce2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)$$
However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ceNO$ and $ceHNO3$:
$$ce3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)$$
Your second reaction equation is obtained by adding these two reaction together.
Reference:
- Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.
Note:
I wrote the $ceH+$ ions as $ceH3O+$, so there is an extra water molecule on the left side of the equation, in each case.
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
add a comment |
Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.
When nitrogen dioxide($ceNO2$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ceHNO3)$ and nitrous acid(HNO2). $$ce2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)$$
i.e.$$ce2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)$$
However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ceNO$ and $ceHNO3$:
$$ce3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)$$
Your second reaction equation is obtained by adding these two reaction together.
Reference:
- Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.
Note:
I wrote the $ceH+$ ions as $ceH3O+$, so there is an extra water molecule on the left side of the equation, in each case.
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
Both of the reactions are correct. However, the second reaction is written by 'adding' two reaction equations.
When nitrogen dioxide($ceNO2$) is dissolved in water, it produces a 1:1 mixture of nitric acid($ceHNO3)$ and nitrous acid(HNO2). $$ce2NO2(g) +H2O(l)->HNO3(aq) +HNO2(aq)$$
i.e.$$ce2NO2(g) +2H2O(l)->H3O+(aq) +NO3-(aq) + HNO2(aq)$$
However, since nitrous acid is unstable in any environment except very cold solution, it decomposes slowly into $ceNO$ and $ceHNO3$:
$$ce3HNO2(aq)->2NO(g) +H3O+(aq) + NO3-(aq)$$
Your second reaction equation is obtained by adding these two reaction together.
Reference:
- Housecroft, C. E.; Constable, E. C. Chemistry, 4th ed.; Pearson, 2010, p 777.
Note:
I wrote the $ceH+$ ions as $ceH3O+$, so there is an extra water molecule on the left side of the equation, in each case.
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
edited Dec 28 '18 at 23:42
orthocresol♦
38.4k7112233
38.4k7112233
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
answered Dec 28 '18 at 21:12
Shoubhik Raj MaitiShoubhik Raj Maiti
1,302530
1,302530
add a comment |
add a comment |
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.
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
add a comment |
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.
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
add a comment |
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.
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
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.
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
answered Dec 28 '18 at 21:09
Oscar LanziOscar Lanzi
14.8k12646
14.8k12646
add a comment |
add a comment |
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