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Consider the daytime production of nitric acid from the reaction of OH. radical and NO2 in...

Consider the daytime production of nitric acid from the reaction of OH^. radical and NO₂ in the gas phase. The chemistry is given below with a rate coefficient of 16 ppbV^-1 min^-1.

OH^. + NO₂ -> HNO₃

During the daytime, OH^. concentration is 4x10^-4 ppbV. If we start with 50 ppbV of nitrogen dioxide and nitrogen dioxide does not get replenished, how much nitric acid has been formed after one hour?

Expert Solution

Reaction :

Assuming elementary reaction,

Rate law is given as:

Integrating with limits

@

# Assuming OH^. remains constant during daytime

Given:

= 4x10^-4 ppbV

= 50 ppbV

= 16 ppbV^-1 min^-1

At t = 1hr (60 min)

Plugging in values:

This is the remaining NO₂

NO₂ consumed = = (50 - 34.05) ppbV

NO₂ consumed = 15.95 ppbV

According to the reaction, 1 mole of NO₂ produces 1 mole of HNO_3.

HNO₃ (nitric acid) produced in 1 hour = 15.95 ppbV

Amanda K answered 7 months ago

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