Hello there, I have this Assignment that is due tommorrow for my chemistry lab,

Question

Hello there,

I have this Assignment that is due tommorrow for my chemistry lab, I need this done as soon as possible.

Thank you very much for your time.

Chemical Equilibrium and Le Chatelier's Principle 6. Reagents: NH,closo, DI water, saturated NH4Cl ago, 12 M HCl Cl (aq) (aq) (EQ 17.18) Hint: sure that the saturated ammonium chloride is saturated (i saturate the reagent container). If not add ammonium chloride to your beaker until is a. Add about 0.5 g of ammonium chloride to a small test tube, wh the test with water. After adding the solid and feel the bottom of temperature change. Record your observations in your Is the solution of ammonium chloride exothermic or endothermico he bottom of out on full tube to note any Write the net ionic equation, putting heat as a reactant or product b. To a second test tube add about 3.0 nL of saturated ammonium chlorid until you see a acid drop wise c. definite test tube, add yourobservations of this change in your lab book 12 Is the reaction shifted to right or the left? Reason for shift. Write the net ionic equation. d. Put the resulting test tube into a hot water bath while stirring mixture the Record your observations. Is the reaction shifted to the right or the left? Reason for shift Write the net ionic equation. e. Put the test tube in ice water. Record your observations. Is the reaction shifted to the right or the left? Reason for the shift. Write the net ionic equation.

Explanation / Answer

Ans a)

Addition of water to ammonium chloride solid in the test tube results in dissolution of ammonium chloride in water and bottom of the test tube feels cooler than the ambient temperature.

Formation of a solution of ammonium chloride in an endothermic process as heat is absorbed from surrounding.

The net ionic equation involving heat can be written as follows:

NH4Cl(s) + heat <===> NH4+(aq)   + Cl-(aq)

--------------------------------------------------------------------------------------------------------------------------------------------------

Ans c)

Observation: temperature of reaction increases.

Addition of con. HCl to saturated solution of ammonium chloride will result in excess concentration of common ion Cl- leading to disturbance in equilibrium. In order to regain the equilibrium, it will shift towards the left side i.e. reactant side. Excess of chloride ions will react with ammonium ions to form ammonium chloride and heat will be given out resulting in higher temperature of the test tube. Net ionic equation can be written as follows:

NH4Cl(s) + heat <=== NH4+(aq)   + Cl-(aq)

-------------------------------------------------------------------------------------------------------------------------------------------------

Ans d)

Observation: more ammonium chloride solid becomes soluble.

Putting the test tube in hot water will result in shift of equilibrium towards right side (forward reaction). Endothermic reactions are favored by increase in temperature. By keeping test tube in hot water, more heat will be available for the reaction and more amount of ammonium chloride will dissociate. Thus, equilibrium will shift to right side dissolving more of ammonium chloride. Net ionic equation can be written as follows:

NH4Cl(s) + heat ===> NH4+(aq)   + Cl-(aq)

-------------------------------------------------------------------------------------------------------------------------------------------------

Ans e)

Observation: more ammonium chloride solid precipitates.

Putting the test tube in cold water will result in shift of equilibrium towards left side(reverse reaction).

Due to lowering of temperature by using cold bath, more of ammonium ions and chloride ions will react to form solid ammonium chloride and heat to maintain equilibrium. Therefore, more solid will precipitate. Net ionic equation can be written as follows:

NH4Cl(s) + heat <=== NH4+(aq)   + Cl-(aq)

Related Questions

Navigate

• Browse (All)
• Browse H
• Subjects

---

---

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