Tipo de Letra (3) Suppose that instead of adding N2, as in (2), you increase the concentration of Hz from 1.00 M (in #1) to 2.00 M, leaving [N2] = 1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? %3D To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16? (4) Can you make a general statement about what happens to a reaction at equilibrium when you add either reactant? How would this be different for a reaction that "goes to completion"?
Tipo de Letra (3) Suppose that instead of adding N2, as in (2), you increase the concentration of Hz from 1.00 M (in #1) to 2.00 M, leaving [N2] = 1.00 M and [NH3] = 4.00 M. Is the system at equilibrium now? If not, which way will the reaction go? First: What would LeChatelier's Principle say? %3D To prove your answer, calculate the new reaction quotient, Qc. Is Qcgreater than, less than, or equal to Kc? (Circle one). If Qc is not equal to Kc, what would have to happen to make it equal 16? (4) Can you make a general statement about what happens to a reaction at equilibrium when you add either reactant? How would this be different for a reaction that "goes to completion"?
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 90AE: In the text, the equation G=G+RTIn(Q) was derived for gaseous reactions where the quantities in Q...
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