Question 2 (a) Consider the following equation NO:(g) + H20(1) – HNO:(aq) + NO(g) (i) Write two balanced half-equations and hence balance the above equation. (ii) Describe the redox behaviour of NO; in this reaction. (iii) State why this reaction is important industrially.
Question 2 (a) Consider the following equation NO:(g) + H20(1) – HNO:(aq) + NO(g) (i) Write two balanced half-equations and hence balance the above equation. (ii) Describe the redox behaviour of NO; in this reaction. (iii) State why this reaction is important industrially.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Solve q2(a=i,ii,ii) part now in 30 min and take a thumb up plz and solve correctly plz according to question.
![Question 2
(a) Consider the following equation
NO:(g) + H2O(1) – HNO:(aq) + NO(g)
(i) Write two balanced half-equations and hence balance the above equation.
(ii) Describe the redox behaviour of NO; in this reaction.
(iii) State why this reaction is important industrially.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe522a9f4-abc6-4fa2-bbd6-740137fb9b1e%2F4478ad60-3689-4016-9bc0-dbaa22161a8a%2Fsicmba_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Question 2
(a) Consider the following equation
NO:(g) + H2O(1) – HNO:(aq) + NO(g)
(i) Write two balanced half-equations and hence balance the above equation.
(ii) Describe the redox behaviour of NO; in this reaction.
(iii) State why this reaction is important industrially.
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