\"In this experiment, you will study the equilibrium conditions of six different

Question

"In this experiment, you will study the equilibrium conditions of six different reactions. You will first establish the equilibrium by mixing the solutions provided for each reaction and then add reagents in order to perturb the established equilibrium. Each time that you cause a change in the equilibrium, you will observe the changes (look for evidence of reaction), write a net ionic equation illustrating the changes and then comment on how the reaction rate is affected, either the forward or reverse reaction rate. The goal is to learn how equilibria respond to changes in concentrations and changes in temperature"

Here is the 6th reaction:

Pretty straight forward, just solve from A through J, each answer takes like one line.

I already did one here is a reference:

6. Reagents: NH Cl (s) DIE water, saturated NH4C1 daqr 12 M HCl aq) NH,C1 Cl NH EQ 17.18) (s) 4 (aq) (aq) Hint: Be sure that the saturated ammonium chloride is saturated (i.e has solid ppt at the bott the reagent container). If not add ammonium chloride to your beaker until Saturate a. Add about 0.5 g of ammonium chloride to a small test tube, which is about on d full with DI water. After adding the solid stir and fee the bottom of the test tu to note any temperature change. Record your observations in your lab book. Is the solution of ammonium chloride exothermic or endolhermic? Write the net ionic equation, putting he as a reactant or prod b. To a second test tube add about 3.0 saturated ammoni loride c. To this test tube, add 12 M hydrochloric acid (CAUTION!) drop wise until you see a definite change. Record your observations of this change in your lab book. Is the reaction shifted to right or the left? Reason for shift. Write the net ionic equation. water bath while stirring the mixture. Record your d. Put the resulting test tube into observations Is the reaction shifted to the right or the left? Reason for shift. te the net ionic equation t tube in ice water. Record your observations. e. Pl Is the reaction shifted to the right or the left? for the shift. Write the net ionic equation.

Explanation / Answer

1) equilibrium expression-

K=[CoCl4]2-/[Co(H2O)6]2+ [Cl-]^4

reaction 6th

K=[NH4Cl]/[NH4+][Cl-] =1/[NH4+][Cl-] as for pure solids concentration=1

2)reverse reaction

rxn 6 -reverse rxn

3) net ionic -

Co2+(aq)+H2O(l) <--->[Co(H2O)6]2+

for rxn 6 -NH4+(aq) +Cl-(aq) <--->NH4Cl(s)

4)by adding 12M HCl same for 6th rxn

5)color change pink to blue   [Co(H2O)6]2++4 [Cl-]   <------>[CoCl4]2- +6H2O(l)

equilibrium is marked by precipitate formation of NH4Cl(s)

6)rxn 6- NH4+(aq) +Cl-(aq) <--->NH4Cl(s)

7)reverse rxn speeds up on addition of product Cl- (HCl)

8)for 6th rxn -hot water that increases solubility of NH4Cl shifting eqm to the right

9) 6th rxn-disappearance of precipitate-clear solution

10)net ionic-NH4Cl(s)<--->NH4+(aq) +Cl-(aq)

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