Question

please help

1. Dinitrogen tetraoxide (colorless gas) is converted to nitrogen dioxide (dark reddish brown gas) and is endothermic in the forward direction: A. Write a balanced equation. B. If a closed container containing a mixture of these two gases at equilibrium is a light brown in color when it is at room temperature (20.0°C), what change would you expect to observe if the container is placed in boiling water (100.0 °C)? c. If a closed container containing a mixture of these two gases at equilibrium is a light brown in color when it is at room temperature (20.0°C), what change would you expect to observe if the container is placed in ice water (0.0 °C)? 2. Hydrogen gas (colorless) reacts with pure iodine vapor (purple) to give hydrogen iodide gas (colorless): A. Write a balanced equation. B. If the equilibrium mixture of these three gases is light purple in color, what change would you expect to observe if more hydrogen gas were added to the system? C. If the equilibrium mixture of these three gases is light purple in color, what change would you expect to observe if some of the hydrogen iodide gas were removed from the system?

Answer 1

A Balanced chemical equation. N204 Colourless gai 2NO, AHive dark redalih broen gas 1 B- me effect of temperature can be explained based on te-Chateliers principle. It states that the change in any of the factors like concentration, temperature pressure et which determine the equilbrium conditions of a system will cause the system to change in such a manner so as to reduce or to counteract the effect of the change. 000) * Conditions given : Light brown in colour at room temperature Change in condition Placed in (100°C). Boi ung water Thus inuease in temperature favours forward reaction, ie forming of No, which can be observed in the form of inueose in colour intensity.ie Intensity of Brown colour inueases. 1.6. Conditions given : Ught brown colour at room temperature 100 Change in condition : Placed in CO°C) Ice Water. The conditions indicate decease in temperature. And since forward reaction is endothermic decrease in temperature would favour reverse reaction le forming N204 This can be observed by decrease in Intensity of brown colour. for an Endothermic Reaction, Conclusion: Thu ease in temperature for a reaction at equilibrium lavours foward reaction whue as decease'm femperature would favour reverse reaction. (Only if it is a Endothermic Reaction) For an Exothermic Reaction, Conclusion: Tnaease in temperature for a reaction at equilibrium favours backward Cor) reverse reaction where as decrease in temperature favours forward reaction Conly if it exothermic reaction)

9.A H + ecotourless) J. (purple) SHI Colourless). 2B. This is based on le-Chottiers priociple. TUIs Based on the effect of change in concertotion OF He is added to the equilibrium veaction mixture, the reaction could shift in forrard direction. According to le-Chartier's prindple, on addition of Hagas, since yeactant concentration is mu easing the reaction will proceed in forward direction to re-estabush equilibrium Thus change in equilibrium le reaction cacering forward direction can be understood in decrease of purple colour intensity 20: Te the hydrogen lodide gas was removed from the system, it would also favour forward reaction og decreasing the concertation of products indicates that the concentration of reactants is more when compared to product) thus to re-establish equilibrium the reaction could favour in forvard direction. This could be obeserved and understood by the decease in the purple colour intensity Conclusion : According to le-Chatiers principle. * Addition of Reactant favours toward reaction * Removal of Product favours forward reaction * Addition of Product favours Reverse reaction * Remowl of Reactant favours Reverse reaction.