If the reactionN2(g) + 3H2(g) = 2NH3(g)is at equilibrium, what direction will the reaction shift if NH3 gas is added?• View Available Hint(s)The reaction will remain unchanged.The reaction will shift to produce both reactants and products.The reaction will shift to produce reactants.The reaction will shift to produce products. If an endothermic reaction is at equilibrium, how will the equilibrium shift when heat is added to the reaction?• View Available Hint(s)The reaction will shift toward the products.The reaction will shift toward both reactants and products.The reaction will shift toward the reactants.The reaction will not shift toward products or reactants.O O O

Answered: Image /qna-images/answer/02973148-9097-40be-a8c4-8e310c88689a.jpg

If the reaction N2(g) + 3H2(g) = 2NH3(g) is at equilibrium, what direction will the reaction shift if NH3 gas is added? • View Available Hint(s) The reaction will remain unchanged. The reaction will shift to produce both reactants and products. The reaction will shift to produce reactants. The reaction will shift to produce products.

If the reaction N2(g) + 3H2(g) = 2NH3(g) is at equilibrium, what direction will the reaction shift if NH3 gas is added? • View Available Hint(s) The reaction will remain unchanged. The reaction will shift to produce both reactants and products. The reaction will shift to produce reactants. The reaction will shift to produce products.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem SI4RE

See similar textbooks

Similar questions

During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. Consider the following exothermic reaction at equilibrium: N2(g)+3H2(g)2NH3(g)Predict how the following changes affect the number of moles of each component of the system after equilibrium is re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
. What does it mean to say that a state of chemical or physical equilibrium is dynamic?
Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
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.
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.)
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.