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Consider the following gas-phase reaction: NO2(9) + N20(g)=3 NO(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>G° w increase, decrease, or not change with increasing temperature from the pulldown menu. T. = 934.9 X K, and AG° will (decrease with increasing temperature. For each of the temperatures listed below calculate AG° for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 454 K AG° = X kJ/mol, and the reaction is --Select-- 9x under standard conditions. (b) At T = 908K AG° = 158 X k)/mol, and the reaction is -Select-- Ox under standard conditions. (c) At T = 1362 K AG° = X kJ/mol, and the reaction is -Select- 9x under standard conditions.

Consider the following gas-phase reaction: NO2(9) + N20(g)=3 NO(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>G° w increase, decrease, or not change with increasing temperature from the pulldown menu. T. = 934.9 X K, and AG° will (decrease with increasing temperature. For each of the temperatures listed below calculate AG° for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 454 K AG° = X kJ/mol, and the reaction is --Select-- 9x under standard conditions. (b) At T = 908K AG° = 158 X k)/mol, and the reaction is -Select-- Ox under standard conditions. (c) At T = 1362 K AG° = X kJ/mol, and the reaction is -Select- 9x under standard conditions.

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Consider the following gas-phase reaction: NO2(9) + N20(g) = 3 NO(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>G° will increase, decrease, or not change with increasing temperature from the pulldown menu. To = 934.9 X K, and AG° will (decrease with increasing temperature. For each of the temperatures listed below calculate AG° for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 454 K AG° = X kJ/mol, and the reaction is (--Select- )x under standard conditions. (b) At T = 908 K AG° = 158 X kJ/mol, and the reaction is -Select-- under standard conditions. (c) At T = 1362 K AG° = x kJ/mol, and the reaction is -Select- Ox under standard conditions.
Transcribed Image Text:Consider the following gas-phase reaction: NO2(9) + N20(g) = 3 NO(g) Using data from Appendix C of your textbook calculate the temperature, To, at which this reaction will be at equilibrium under standard conditions (AG° = 0) and choose whether A>G° will increase, decrease, or not change with increasing temperature from the pulldown menu. To = 934.9 X K, and AG° will (decrease with increasing temperature. For each of the temperatures listed below calculate AG° for the reaction above, and select from the pulldown menu whether the reaction under standard conditions will be spontaneous, nonspontaneous, or near equilibrium ("near equilibrium" means that T is within 5 K of To). (a) At T = 454 K AG° = X kJ/mol, and the reaction is (--Select- )x under standard conditions. (b) At T = 908 K AG° = 158 X kJ/mol, and the reaction is -Select-- under standard conditions. (c) At T = 1362 K AG° = x kJ/mol, and the reaction is -Select- Ox under standard conditions.
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