Thanks in advance :) 1. Assume that the following reaction is in chemical equili

Question

Thanks in advance :)

1. Assume that the following reaction is in chemical equilibrium: N2(g) + 3H2(g) 2 NH3(g) + heat Use Le Chatelier?s Principle to explain the effect each of the following changes will have upon the System - will the equilibrium shift toward the product or reactant side? Why?? a. If more hydrogen is added to the system the equilibrium will shift to the (circle one and explain below) i. Right ii. Left iii. Remains unchanged b. If ammonia is removed from the system the equilibrium will shift to the (circle one and explain below) i. Right ii. Left iii. Remains unchanged c. If nitrogen is removed from the system the equilibrium will shift to the (circle one and explain below) i. Right ii. Left iii. Remains unchanged d. If the temperature is raised the equilibrium will shift to the (circle one and explain below) i. Right ii. Left iii. Remains unchanged e. If the pressure of the system is decreased by doubling the total volume the equilibrium will shift to the: (circle one and explain below) i. Right ii. Left iii. Remains unchanged

Explanation / Answer

a) To right as we are adding reactant and reaction will go in the direction where the effect can be nullified.

b) ammonia is removed = the reaction will move towards right in order to produce more ammonia

c) Nitrogen removed = equilbirium will move left to add on nitrogne to the system

d) it is exothermic so temperature increase will shift reaciton towards left

e)an increase in the total pressure on the system. The reaction then shifted in the direction that minimized the effect of this stress. The reaction shifted toward the products because this reduces the number of particles in the gas, thereby decreasing the total pressure on the system,

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.