Ex p e ri m e n t L e Chatelier’s P r i n c i pl e Le Chatelier’s Principle Ange

Question

Experiment   Le Chatelier’s Principle

Le Chatelier’s Principle

Angela Carraway, Ph.D. & Peter Jeschofnig, Ph.D. Version 42-0166-00-01

Lab Report Assistant                                                                                            

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor.

Questions                                                                                                                 

Part I

2+

In Part I the reaction you observed was Mg(OH)2 (s) ó Mg

(aq) + 2 OH- (aq). Compare the colors

you observed in the experiment and answer these questions:

A. Which way should the equilibrium shift when HCl is added? How do your results support your answer?

B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?

C. Is this reaction endothermic or exothermic? How do you know?

Part II

In Part II the reaction you observed was HSO4 (aq) + H2O (l) ó H3O (aq)+SO4

. Compare the colors

-                                                                  +                            2-

you observed in the experiment and answer these questions:

A. Which way should the equilibrium shift when Na2SO4 is added? How do your results support your answer?

B. Which way should the equilibrium shift when NaHSO4 is added? How do your results support your answer?

C. Is this reaction endothermic or exothermic? How do you know?

2+

Explanation / Answer

Mg(OH)2 (s) <--> Mg+2(aq) + 2 OH- (aq).

A. Which way should the equilibrium shift when HCl is added? How do your results support your answer?

If you add HCl, H+ ions will react with OH- ions, therefore, the product concnetration decreases and the equilibrium shifts toward PRODUCTS

B. Which way should the equilibrium shift when Na2EDTA is added? How do your results support your answer?

When Na2EDTA is added to the solution, EDTA-2 reacts with Mg+2

the products concentration lowers, the shift goes toward products

C. Is this reaction endothermic or exothermic? How do you know?

Mg+2 and EDTA-2 will react and will cool the syste, therefore, it is endothermic

NOTE:

consider posting all other questions in another set of Q&A. Wea re not allowed to answer to multiple questions in asingle set

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