# chemistry

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Calculatet the solubility of silver chloride in a 0.10 mol/L solution of sodium chloride at 25 degrees celsius.At SATP, Ksp AgCl(s) = 1.8 x 10^-10

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Refer to the post by Marcus just eight (8) questions below your post.

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How will the removal of some HOCl(g) from the following system affect the equilibrium?

H2O(g) + Cl2O(g) HOCl(g)

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You don't have an arrow. I can't tell the difference between reactants and products.

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How will the removal of some HOCl(g) from the following system affect the equilibrium?

H2O(g) + Cl2O(g)----> HOCl(g)

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Remember what Le Chatelier's Principle says. It says that when a system in equilibrium is subjected to a stress, the equilibrium (the reaction) will shift is such a way so as to remove the stress. So let's analyze what is happening. If we remove some HOCl from the system, the reaction must shift so as to do what? It must replace some of what is being removed. How can it do that? With H2O and Cl2O reacting to produce more HOCl to replace what was removed. So the reaction must shift to the right. In practical terms, that means some H2O is used, some Cl2O is used (both will decrease in concentration) and some HOCl is produced (although the HOCl probably will not get as high as it was before some was removed initially).

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If 1.00 mol of each of carbon dioxide and hydrogen is initially injected into a 10-L reaction chamber at 986 degrees celsius, what would be the concentrations of each entity at equilibrium?

CO2(g) + H2(g)<---> CO(g) + H2O(g)

k = 1.60 for 986 degrees celsius

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You should repost this as a separate post. Posts posted as a piggy back onto another question tend to get lost.