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The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,
is 1.3 x 106 and that for
is 6.5 x 10-16 (when each species is expressed in terms of partial pressure).
For the reaction,
equilibrium constant is
- a)
- b)
- c)
- d)
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
The concentration of the oxides of nitrogen are monitored in air-pollu...
Given equations are
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
Most Upvoted Answer
The concentration of the oxides of nitrogen are monitored in air-pollu...
Given equations are
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
NO (g) + ½ O2 (g) ⇌ NO2 (g) ----------(i) k1 = 1.3×106
And ½ N2 (g) + ½ O2 (g) ⇌ NO(g) ----------(ii) k2 = 6.5×10-16
To get the reaction, N2(g) + 2O2(g) ⇌ 2NO2(g) ----------(iii) k3
We multiply eqn (i) and eqn (ii) by 2 and adding both reaction, we get eqn (iii)
k3 = k12×k22
= (1.3×106)2×(6.5×10-16)2
= 1.69×1012×42.25×10-32
= 7.14×10-19
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The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer?
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The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer?.
The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? for Class 11 2025 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for Class 11 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer?.
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The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer?, a detailed solution for The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? has been provided alongside types of The concentration of the oxides of nitrogen are monitored in air-pollution reports. At 25°C, the equilibrium constant for the reaction,is 1.3 x 106 and that foris 6.5 x 10-16 (when each species is expressed in terms of partial pressure).For the reaction,equilibrium constant isa)b)c)d)Correct answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
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