Question #f8f8f

1 Answer
Jun 28, 2017

Answer:

#2"NO"_ ((g)) + "O"_ (2(g)) -> 2"NO"_ (2(g))#

Explanation:

Nitric oxide, #"NO"#, reacts with oxygen gas to produce nitrogen dioxide, #"NO"_2#, according to the following unbalanced chemical equation

#"NO"_ ((g)) + "O"_ (2(g)) -> "NO"_ (2(g))#

To balance the chemical equation, start by multiplying the nitric oxide by #2# to get

#2"NO"_ ((g)) + "O"_ (2(g)) -> "NO"_ (2(g))#

At this point, you have #2# atoms of nitrogen and #4# atoms of oxygen on the reactants' side and only #1# atom of nitrogen and #2# atoms of oxygen on the products' side, so multiply the nitrogen dioxide by #2# to get the balanced chemical equation

#2"NO"_ ((g)) + "O"_ (2(g)) -> 2"NO"_ (2(g))#

http://www.chegg.com/homework-help/questions-and-answers/entropy-decreases-g-oxidized-o2-g-no2-g--major-factor-leads-decrease-entropy-reaction-show-q6986757