Problem: At 1 atm and 25 °C, NO2 with an initial concentration of 1.00 M is 3.3 × 10−3% decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction.2NO2(g) ⇌ 2NO(g) + O2(g)

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FREE Expert Solution

We are being asked to calculate the equilibrium constant, Kc for the given equilibrium reaction:

2NO2(g) ⇌ 2NO(g) + O2(g)


When dealing with equilibrium and Kc:

Kc → equilibrium units are in molarity 
Kc is an equilibrium expression:

Kc=productsreactants

only aqueous and gaseous species are included in the equilibrium expression
▪ the coefficient of each compound in the reaction equation will be the exponent of the concentrations in the equilibrium expression


Given:    

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Problem Details

At 1 atm and 25 °C, NO2 with an initial concentration of 1.00 M is 3.3 × 10−3% decomposed into NO and O2. Calculate the value of the equilibrium constant for the reaction.

2NO2(g) ⇌ 2NO(g) + O2(g)

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Based on our data, we think this problem is relevant for Professor Liu's class at PITT.

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.