1. The production of ammonia gas from hydrogen and nitrogen gas is provided below: N₂ (g) + 3 H₂ (g) = 2 NH3(g) AH = -92 kJ/mol a) Sketch a Concentration vs Time graph that shows some initial amount of N₂ and H₂ reacting to produce NH3 from an initial amount of 0 up to an equilibrium being established. Label initial, change and equilibrium on your sketch. b) Once equilibrium is reached, suggest 2 ways to increase the amount of NH3. Explain your reasoning using Le Chatelier's principle.

1. The production of ammonia gas from hydrogen and nitrogen gas is provided below: N₂ (g) + 3 H₂ (g) = 2 NH3(g) AH = -92 kJ/mol a) Sketch a Concentration vs Time graph that shows some initial amount of N₂ and H₂ reacting to produce NH3 from an initial amount of 0 up to an equilibrium being established. Label initial, change and equilibrium on your sketch. b) Once equilibrium is reached, suggest 2 ways to increase the amount of NH3. Explain your reasoning using Le Chatelier's principle.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.100PAE: 12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial...

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12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
A 100.-gram sample of sodium chloride (NaCl) is added to 100. mL of water at 0 C. After equilibrium is reached, about 64 g of solid remains undissolved. Describe the equilibrium that exists in this system at the particulate level.
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 45 s? After 90 s?
. Explain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?
For the endothermic reaction AB(g)A(g)+B(g), the following represents a reaction container at two different temperatures. Which one (I or II) is at the lower temperature?
Consider the reaction A+BC+D. A friend asks the following: “I know we have been told that if a mixture of A, B, C. and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?” What do you tell your friend?
. Equilibrium may be defined as the ________ of two processes, one of which is the opposite of the other.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
In each of the reactions, how does the equilibrium respond to an increase in pressure? (a) 2SO 2 ( g )+ O 2 ( g ) 2SO 3 ( g ) (b) H 2 ( g )+ I 2 ( g )2HI( g ) (c) 3H 2 ( g )+ N 2 2NH 3 ( g )