# 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:

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

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:

###### 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)

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the ICE Chart concept. You can view video lessons to learn ICE Chart. Or if you need more ICE Chart practice, you can also practice ICE Chart practice problems.

What professor is this problem relevant for?

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

What textbook is this problem found in?

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.