HClO(aq) +H2O ==> H3O+(aq) +ClO-(aq)
a)
Removing some HClO(aq)
According to le chatlier's principle
As we removed HClO, equilibrium is distributed so to attain equilibrium the change occurs reverse to that of original change
So
As removing HClO we decreased the concentration of HClO so the equilibrium shifts to left side I.e reactants side to increase the concentration and re attain the equilibrium
( shifts in the direction of the reactants)
b)
Adding more ClO-
As we added more ClO- the concentration of ClO- increased so the equilibrium shifts to the left side I.e reactants side to decrease the concentration of ClO- by forming more amount of reactants
(shifts in the direction of the reactants)
C)
Removing some H3O+
As we removed H3O+ the concentration of H3O+ is decreased so the equilibrium shifts to the right side I.e products side to increase the concentration of H3O+
(shifts in the direction of the products)
D)
Adding more HClO
As we added more HClO the concentration of HClO is increased so the equilibrium shifts to the right side I.e the products side to decrease the concentration of HClO by forming more amount of products
(shifts in the direction of the products)
20. Use Le Châtelier's principle to predict if each of the following changes causes the system to shift in the dire...
Use LeCha^telier′s principle to predict whether each the following changes causes the system to shift in the direction of products or reactants: HF(aq)+H2O(l)⇌F−(aq)+H3O+(aq) Part A adding some F−(aq) adding some a.in the direction of the reactants b.in the direction of the products Part B. removing some HF(aq) removing some in the direction of the products in the direction of the reactants SubmitRequest Answer Part C removing some H3O+(aq) removing some in the direction of the products in the direction of...
Use "Le Chatelier's" principle to predict whether each of the following changes causes the systems to shift in the direction of the products (C, D) or reactants (A, B)" A + B -----> <------ C + D a) adding more A b) removing some C c) adding more D d) removing some A
NAMIN SEC Question 4 of 14 > Use Le Châtelier's principle to predict how the equilibrium for the weak base methylamine responds to the indicated chan CH, NH, (aq) +H,0(1) - CH NH; (aq) + OH(aq) AH n = 103 kJ/mol Produces more reactants No change Produces more products Answer Bank increasing the temperature adding CH NH,BE adding KB adding HB adding KOH
8.53 Use Le Châtelier's principle to predict the direction of equi- librium shift and the changes that will be observed (color, amount of precipitate, etc.) in the following equilibria when the indicated stress is applied: a. heat +Co2 (aq) +4CI (aq)2 COCL (aq); colorless blue pink The equilibrium mixture is heated. b.heat+Co2 (aq) + 4CI (aq)e CoCL (aq); blue pink is added to the equilibrium mixture. colorless Co c. Fe3 (aq) + 6SCN (aq) Fe(SCN),(aq); red brown colorless SCN is...
For the following equilibrium reaction, predict the direction of the equilibrium shift by specifying if each stress will cause the concentration of reactants or products to increase NH3(g)+H2O(l) ⇋ NH4+(aq)+OH−(aq) Drag the appropriate stresses to their respective bins. Adding NH4+(aq) Adding NH3(g) Adding OH-(aq) Removing NH4+(aq) Removing OH-(aq) Shifts in the direction of the reactants: Shift in the direction of the products:
Le Chatelier's Principle 3. For Part Ill, use Le Châteller's Principle to explain the colour changes observed in test tubes 2 and 3 upon the addition of HC and A . Also, explain the observed colour changes in the test tubes placed in hot and cold water. (4 marks) Test Tube 2: Test Tube 3: Hot Water bath: Cold Water bath: Extension: 1. NaCl(aq) + HCl(aq) = NaCl(aq) + H2O + Cl2(g) When the above system is cooled, gas bubbles...
NaOH is added to the following reaction: NH4+(aq) + H2O(l)-->H30+(aq)+NH3(aq) Using Le Châtelier's Principle, state in which direction the equilibrium will shift in response to the change. Briefly defend your answer.
Le Chateler's principle In the chart below: • Indicate the color of each solution as darker or lighter than the control after the addition of the specified substance. • Indicate the direction the equilibrium shifted as "toward products" or "toward reactants" based on the color change. • Based on the direction of the shift, indicate the substance(s) that increased which will either be the two reactants present on the reactant side of the equilibrium equation or the complex present on...
4. Consider the following system at equilibrium: a. According to Le Châtelier's Principle, what effect will increasing the amount of reactant A have upon the amount of product C? Will it increase the amount of C or decrease the amount of C? b. In which direction did this increase in the amount of A shift the equilibrium? To the left, or to the right? 5. Consider the following system at equilibrium: a. According to Le Châtelier's Principle, what effect will...
1) The reaction below is exothermic 2SO2 (g) + O2(g) ⇌ 2SO3(g) + heat Le Châtelier's Principle predicts that _______ will result in an increase in the number of moles of SO3 (g) in the reaction container. Which direction will the reaction shift: ? left or right A) increasing the volume of the container B) increasing the amount of SO2 C) removing some oxygen D) increasing the temperature E) decreasing the pressure 2) Consider the following reaction at equilibrium: 2SO2 (g) + O2 (g) ⇌ 2SO3 (g) + heat ΔH...