an endothermic reaction.

Anonymous

Discussion:

The first experiment suggests that the decomposition of N2O4 is an endothermic reaction. This is because when

Anonymous

Discussion:

The first experiment suggests that the decomposition of N2O4 is an endothermic reaction. This is because when the equilibrium mixture was heated, the color changed from light brown to dark brown. That means that more N2O4 was formed. Since it proceeds in the forward direction with the addition of heat, the reaction is thus endothermic.

The second part validates our results in the first part. Placing the gas mixture in a colder environment changes the color of the gas from light brown to colorless. That means that more N2O4 was formed. Proceeding the reverse reaction when lowering the temperature indicates an endothermic reaction.

The third part is an additional validation for the first two. Increasing the pressure changes the color of the gas from light brown to colorless again. That means that more N2O4 was produced indicating that it went to the direction where there is less moles of gas a result of increasing the pressure.

For the Haber reaction, since we initially started with just the reactants, it is imperative that the reaction will proceed forward. This means that more ammonia gas will be formed which will then react with the fluid indicator turning it to the pink. The pink just indicates the formation of a basic solution which is from the ammonia.

Conclusion:

This experiment aimed to demonstrate the concept of Le Chatelier’s principle. For the decomposition of N2O4 to NO2, it was found out that it is an endothermic reaction. That means that increasing the temperature in the mixture favors the forward reaction. The Haber process also shows that if there is an absence of products or there are only reactants in the mixture, it is imperative that it will move in the forward direction to maintain equilibrium.

was heated, the color changed from light brown to dark brown. That means that more N2O4 was formed. Since it proceeds in the forward direction with the addition of heat, the reaction is thus endothermic.

The second part validates our results in the first part. Placing the gas mixture in a colder environment changes the color of the gas from light brown to colorless. That means that more N2O4 was formed. Proceeding the reverse reaction when lowering the temperature indicates an endothermic reaction.

The third part is an additional validation for the first two. Increasing the pressure changes the color of the gas from light brown to colorless again. That means that more N2O4 was produced indicating that it went to the direction where there is less moles of gas a result of increasing the pressure.

For the Haber reaction, since we initially started with just the reactants, it is imperative that the reaction will proceed forward. This means that more ammonia gas will be formed which will then react with the fluid indicator turning it to the pink. The pink just indicates the formation of a basic solution which is from the ammonia.

Conclusion:

This experiment aimed to demonstrate the concept of Le Chatelier’s principle. For the decomposition of N2O4 to NO2, it was found out that it is an endothermic reaction. That means that increasing the temperature in the mixture favors the forward reaction. The Haber process also shows that if there is an absence of products or there are only reactants in the mixture, it is imperative that it will move in the forward direction to maintain equilibrium.

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