-1 -Chem. Eq Chemical Equilibrium Purpose of the Experiment Observe the effects
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Question
-1 -Chem. Eq Chemical Equilibrium Purpose of the Experiment Observe the effects of disturbances on three chemical systems at equilibrium. Consider these effects in relation to Le Chatelier's principle. You should be familiar with basic laboratory techniques for transferring solids, mixing solutions, and using hot-and ice-water baths. You should also be familiar with the concepts associated with stoichiometry and thermochemistry. Background Information Many chemical reactions do not proceed to completion. The reaction shown in a typical chemical equation is called the forward reaction (the arrow points to the right or the product side of the reaction). In many cases, the reaction products begin reacting to re-form the original reactants, while the forward reaction is still going on. We call this reverse process the reverse or backward reaction. Ultimately, under the right conditions, the rates of the forward and backward reactions become equal. At this point, the concentrations of reactants and products stabilize, and we say that the chemical system has reached equilibrium. When writing the chemical equation for a system at equilibrium, we use double arrows to indicate the simultaneous occurrence of forward and reverse reactions. We call reactions that behave in this way reversible. Disturbances that alter the concentration of any species in a system at equilibrium necessarily disturb that equilibrium. We can predict the response of a chemical equilibrium to such disturbances by using Le Chatelier's principle. This principle states that a chemical system at equilibrium responds to a change in conditions by adjusting the relative concentrations of the reaction components to relieve the effects of that change. The adjustment, or shifting, continues until a new equilibrium is established, at which point the rates of the forward and reverse reactions are once again equal. Chemical equilibria also respond to temperature and other changes, although such responses are not included in the chemical equations for the equilibria. For example, an exothermic reaction at equilibrium will respond to a temperature increase by increasing the concentration of reactants, in order to adjust to the added heat.Explanation / Answer
1. a) i) One should remember that 12 M HCl ie concentrated HCl is too much fuming in nature. So high chances are there to inhale the vapour which can damage internal organ. Sometimes this internal organ damage is fatal.
ii) Concentrated HCl is corrosive in nature. So it can cause the irritation in skin, eye etc. So concentrated HCl(12 M) should be handled with care.
b) i) 0.1M CoCl2 in 95 % ethanol is toxic and carcinogenic.
ii) It's an allergen. It causes eye and skin irritation. So one should be very careful from skin contact.
iii) It's harmful if swallowed as it may interfere in blood clotting, it can cause also thyroid abnormalities and delayed lung injury.
iv) It's harmful for environment. So one should dispose this chemical properly after use for experiment.
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