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g) If the reaction was carried out at 200°C instead, the concentrations of the ammonia and the carbon dioxide were lower than when the reaction was carried out 250°C. Use this information to determine if the reaction is endothermic or exothermic, and be sure I can follow your reasoning (try to be concise, please!).

g) If the reaction was carried out at 200°C instead, the concentrations of the ammonia and the carbon dioxide were lower than when the reaction was carried out 250°C. Use this information to determine if the reaction is endothermic or exothermic, and be sure I can follow your reasoning (try to be concise, please!).

Chemistry
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I just need help with part g please

 

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Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature.
Transcribed Image Text:Consider the reaction: NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) At high temperatures such as 250.°C, the equilibrium constant for the reaction is 1.58 x 10-8. A research student ran the experiment by first placing 39.1 g of the reactant compound in a 750. mL evacuated closed container. (R = 0.08206 L.atm/K.mol; K = °C + 273; pay attention to sig figs) a) Write the equilibrium expression, Kc, for this reaction. kc=l.58 x 10 COONH kc [NH3]? [COz] b) What is the concentration of each of the products at equilibrium? NH2COONH4 (s) = 2 NH3 (g) + CO2 (g) NHz COON H4: 39.1g 78.070 gimol 50 mol NH2 COON Hy = Z NH3 CO2 Tnitial -50 gimo1 W 999. + 2 X t ズ ミGGG N •150L E : 666-X answer: ENHS] = 2(-89x104) :1.78x10-4 M C COz] = -89x 10 4 M kc CNH3]?CCO1] →1.58* 10°8-(2x) Cx) 2x2.1.58x 1 X: 1.58x108 c) What is the pressure in atm exerted by each of the products at equilibrium? on 79x 10 こ、 kp= kc x (RT) X= .89x104 R=. 08206 kp:1.58x10-8 x(.08206x523)? :1,58 x 108x (42.91738)? : 2.9|x 10-5 n (3-1) = 2 入 T 523 k -5 [NH3]=2(,0302) = . O605 altm X= .0302 COL): 10302 atm d) Use these pressures to calculate the Kp for the reaction at this temperature.
g) If the reaction was carried out at 200°C instead, the concentrations of the ammonia and the carbon dioxide were lower than when the reaction was carried out 250°C. Use this information to determine if the reaction is endothermic or exothermic, and be sure I can follow your reasoning (try to be concise, please!).
Transcribed Image Text:g) If the reaction was carried out at 200°C instead, the concentrations of the ammonia and the carbon dioxide were lower than when the reaction was carried out 250°C. Use this information to determine if the reaction is endothermic or exothermic, and be sure I can follow your reasoning (try to be concise, please!).
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