Why does a system in equilibrium appear, on a macroscopic level, as if no change

Question

Why does a system in equilibrium appear, on a macroscopic level, as if no change is taking place? In the body, an equilibrium exists between calcium, phosphate ions, and calcium phosphate, which is a major constituent of kidney stones. Explain why a large increase in health problem. 3Ca^2+ (aq) + 2PO_4^3+ (aq) Ca_3 (PO_4)_2 (s) The production of hydrogen gas can be accomplished by reacting carbon monoxide with water vapor. This reaction establishes the following equilibrium. Predict the shifts in equilibrium that accompany each of the conditions according to lessthanorequalto Chatelier's principle. CO(g) + H_2 O(g) H_2 (g) + CO_2 (g) + 9.9 kcal a. Increase in CO(g) concentration b. Decrease in temperature c. Removal of the H_2 (g) d. Increase in pressure

Explanation / Answer

Q1.

In a macroscopic level, there are no changes in overall concentrations, since the changes and rates in equilibrium are very fast, so the change in AVERAGE change with respect to "dt" or time, are neglegible

Q2

The equation appears to have:

ions of Ca+2 and ions of PO4-3

increasing Ca+2 will increase the reagetns, therefore the euqilibrium tends to shift towards product

the product being the solid form of the "kideney stones"

Q3

a)

increasing CO, a reactant, will favour MORE product formation, due to lechatelier principles

b)

decreasing T, will take off energy, this is endothermic, so it will not favour production, rather reactants (shift goes to left)

c)

Removing H2, a product, will favour even more produciotn of producs in order to counter balance the H2 lodss

d)

Increse in P favour only the least mol of gases formation

in this case, 2 mol of gas = 2 mol of gas so no effeect whatsoever

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