Please help with these chemistry questions, nobody can figure them out. The answers selected are not correct. # Understanding the Equilibrium Between Dinitrogen Tetroxide and Nitrogen DioxideDinitrogen tetroxide and nitrogen dioxide are two gases existing in equilibrium across different temperatures. Nitrogen dioxide (\(NO_2\)) is a reddish-brown gas, while dinitrogen tetroxide (\(N_2O_4\)) is colorless. ### Visual Representation:- **Image Descriptions**: - **Left Image**: Displays a strong red color at high temperature due to \(NO_2\). - **Right Image**: Shows a diminished red color at low temperature as the equilibrium shifts toward the colorless \(N_2O_4\).### Chemical Equilibrium Equation:\[ 2 \, NO_2(g) \rightleftharpoons N_2O_4(g) \]### Conclusions:1. **Nature of Reaction**: - The reaction is **exothermic**.2. **Effect of Temperature on Equilibrium Constant \((K)\)**: - When temperature decreases, the equilibrium constant: - **Decreases**.3. **Effect of Temperature on Equilibrium Concentration of \(N_2O_4\)**: - When temperature decreases, the equilibrium concentration of \(N_2O_4\): - **Increases**.This analysis helps understand the temperature-dependent behavior of gaseous equilibria and the observable color changes as an indication of such shifts. ### Dinitrogen Tetraoxide and Nitrogen Dioxide EquilibriumDinitrogen tetraoxide \((\text{N}_2\text{O}_4)\) and nitrogen dioxide \((\text{NO}_2)\) are two gases that exist in equilibrium over various temperatures. \(\text{NO}_2\) is a reddish-brown gas, whereas \(\text{N}_2\text{O}_4\) is colorless.#### Visual Representation:- **High Temperature:** The red color is strong, indicating a higher concentration of \(\text{NO}_2\).- **Low Temperature:** The gas has less color, indicating a higher concentration of \(\text{N}_2\text{O}_4\).#### Chemical Equilibrium:The equilibrium can be represented as:\[ 2 \text{NO}_2(g) \rightleftharpoons \text{N}_2\text{O}_4(g) \]#### Conclusion:1. **This reaction is:** - \( \circ \) Exothermic. - \( \bullet \) Endothermic. - \( \circ \) Neutral. - \( \circ \) More information is needed to answer this question.2. **When the temperature is increased, the equilibrium constant, \( K \):** - \( \circ \) Increases. - \( \bullet \) Decreases. - \( \circ \) Remains the same. - \( \circ \) More information is needed to answer this question.3. **When the temperature is increased, the equilibrium concentration of \(\text{N}_2\text{O}_4\):** - \( \circ \) Increases. - \( \bullet \) Decreases. - \( \circ \) Remains the same. - \( \circ \) More information is needed to answer this question.

Answer:Le-chatalier's principle states that on changing any parameter of the system, reaction shifts in the direction where effect of that change gets eliminated.Given reaction:Since, N2O4 is colorless and NO2 has reddish brown color, it means as the reaction proceeds in forward direction intensity of color decreases and since, at the equilibrium, both the gases are present, therefore color of reaction mixture at the equilibrium should be yellowish and more the reaction moves in forward direction more the intensity of color decreases.Since, it is mentioned that, at low temperature color of the reaction mixture is yellow and at the high temperature, it is red, that means, on increasing the temperature reaction moves in reverse direction and on decreasing the temperature reaction moves in forward direction and according to Le-chatalier's principle, decrease in temperature favors the forward reaction when reaction is exothermic in nature. So, it is an exothermic reaction.Given reaction:Since, it is an exothermic reaction therefore on increasing the temperature, value of equilibrium constant will decrease and reaction will favor the formation of more and more reactants.Given reaction:Since, it is an exothermic reaction therefore value of equilibrium constant will decrease and reaction will favor the formation of more and more reactants and since, N2O4 is a product, so, on increasing the temperature, N2O4 concentration decreases.