Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide.A chemical engineer studying this reaction fills a 125.L tank at 13.°C with 16.mol of nitrogen dioxide gas. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 6.9mol of nitrogen dioxide gas.The engineer then adds another 8.0mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.

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Asked Mar 5, 2019
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Nitrogen dioxide is one of the many oxides of nitrogen (often collectively called "NOx") that are of interest to atmospheric chemistry. It can react with itself to form another form of NOx, dinitrogen tetroxide.

A chemical engineer studying this reaction fills a 125.L tank at 13.°C with 16.mol of nitrogen dioxide gas. He then raises the temperature considerably, and when the mixture has come to equilibrium determines that it contains 6.9mol of nitrogen dioxide gas.

The engineer then adds another 8.0mol of nitrogen dioxide, and allows the mixture to come to equilibrium again. Calculate the moles of dinitrogen tetroxide after equilibrium is reached the second time. Round your answer to 2 significant digits.

 

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Expert Answer

Step 1

For the given reaction, the equation for equilibrium constant can be written as above.

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Step 2

As the reaction proceeds, it attains equilibrium. The initial concentration of NO2 and the concentration of NO2 at equilibrium can be calculated as given.

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Step 3

Two moles of NO2 reacts to form one mole of  N2O4. Hence, concentration of N2O4 formed will be the half of the concentration o...

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