What would be the impact to equilibriumif by increasing pressure? Which direction wouldthe reaction to progress to get back to equilibrium,and why? For the reaction:H₂O(l)2NH3(g) + CO2(g) = (NH2)2CO(s) +ΔΗ = – 330 kJ==Predict how each of the following changes wouldimpact a reaction that is currently at equilibrium.That is, which way would the reaction progress inorder to respond to the change in the system toregain equilibrium (use arrows to show thedirection of change that would occur to return backto equilibrium). Explain your reasoning for eachpart.

Answer: According to Le-chatalier's principle on changing any parameter of the system that is at…

Answered: For the reaction: H₂O(l) 2NH3(g) +…

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For the reaction: H₂O(l) 2NH3(g) + CO₂(g) = (NH₂)2CO(s) + AH = - 330 kJ

Chemistry

10th Edition

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.

Question

What would be the impact to equilibrium
if by increasing pressure? Which direction would
the reaction to progress to get back to equilibrium,
and why?

For the reaction:
H₂O(l)
2NH3(g) + CO2(g) = (NH2)2CO(s) +
ΔΗ = – 330 kJ
==
Predict how each of the following changes would
impact a reaction that is currently at equilibrium.
That is, which way would the reaction progress in
order to respond to the change in the system to
regain equilibrium (use arrows to show the
direction of change that would occur to return back
to equilibrium). Explain your reasoning for each
part.

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