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A mixture of 4.76 mol N 2 and 30.45 g NO is heated in a closed vessel to 2000 °C. After heating, the total pressure of the mixture at equilibrium is 3.14 atm . N 2 ( g ) + O 2 ( g ) − ⇀ ↽ − 2 NO ( g ) K p = 0.101 at 2000 ° C In which direction does the reaction proceed after heating to 2000 °C? The reaction is at equilibrium. The reaction proceeds toward the reactants. The reaction proceeds toward the products.

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Answer:

- The reaction proceeds toward the reactants as nitrogen monoxide will allow the formation of oxygen.

Explanation:

Hello,

For the given reaction, is it noticed that no change in moles for the reaction, will imply that the equilibrium pressure equals the initial pressure:

[tex]p_T^{eq}=p_0^{eq}=3.14atm[/tex]

Nonetheless, since at beginning there is no oxygen, it is clear that the reaction must be:

[tex]2 NO \rightleftharpoons N_2 ( g ) + O_2 ( g )[/tex]

In such a way, since the initial mixture contains both nitrogen monoxide and nitrogen, the nitrogen monoxide will be the reactant, therefore the reaction WILL HAVE TO MOVE TOWARDS PRODUCTS, that is to oxygen and nitrogen, in order to attain equilibrium. Hence, the answer will depend on:

- If the reaction is:

[tex]N_2 ( g ) + O_2 ( g )\rightleftharpoons 2 NO[/tex]

The reaction proceeds toward the reactants as nitrogen monoxide will allow the formation of oxygen.

- If the reaction is:

[tex]2 NO \rightleftharpoons N_2 ( g ) + O_2 ( g )[/tex]

The reaction proceeds toward the products as nitrogen monoxide will allow the formation of oxygen.

Finally, as the initial reaction is:

[tex]N_2 ( g ) + O_2 ( g )\rightleftharpoons 2 NO[/tex]

The answer is: the reaction proceeds toward the reactants.

Best regards.

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