What are 2 examples of chemicals that you can use to shift the equilibrium in a reaction involving cobalt(II)?
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Anything, at this point... once you add something reactive to the cobalt, the reaction will turn reactants (cobalt and ____) into products, shifting the equillibrium.\n\nCobalt two has a positive-two charge.  You should add any ion with a negative-two charge: carbonate (CO3), chromate (CrO4), dichromate (Cr2O7), an oxide (O), sulfate (SO4), sulfide (S), or sulfite (SO3).
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go to\nwww.chemistry.com
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2NaOH + CO2 = Na2CO3 + H2O
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Cobalt cyanide. Read all about it here:
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Try doing a Google search under the Hall or the Hall-Heroult process.    That or check out a General or an Inorganic Chemistry book from the library.  That's a good launch point.
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Na2CO3 + 2HCl = CO2 + H20 + 2NaCl (aq)\n\nThis reaction is a double displacement reaction because oxygen from the sodium carbonate combines with the hydrogen in the hydrochloric acid to form water, and the sodium goes with chlorine to form sodium chloride, making carbon dioxide in the process.
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Candidates include ammonium carbonate, (NH4)2CO3, or polymers where two CO groups get bridged by one NH.
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cobalt can be used just about anywhere iron could. the primary place would probably use in magnets
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2Ag+ + CO_33-2 -> Ag_2CO_3
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CH3COOH + NaOH ---> NaCH3COO + H2O
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2K + I2 -> 2KI\n\nBa + S -> BaS\n\nMgBr2 + MnI6 -> No Reaction\n\nC7H16 + H2O -> No Reaction\n\n2KI + Br2 -> 2KBr + I2
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1.  Split up the elements and give them their original charges\n\nAg +\nNO3 -\nK +\nBr -\n\n2.  Combine an element with an element that they were not with, putting them side by side will help\n\nAg + with Br -\nNO3 - with K +\n\n3. So now you have 2 new compounds\n\nAgBr & KNO3-\n\n4.  Their should be a chart in your book that tells you which compound would be the precipitate but i don't think their is a precipitate for this reaction'\n\nso both will dissolve in a solution
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5.  K = [NH3][HCl] = (0.066 M)^2 = 4.36 x 10^-3\n\n9.  I'm assuming that equation should be H2(g) + CO2(g) <---> H2O(g) + CO (g)\na.  Add H2O will drive equlibrium to the left\nb.  Removing CO will drive equilibrium to the right\nc.  Adding H2 will drive equilibrium to the right\nd.  Adding something to absorb CO2 will drive equilibrium to the left\n\n6. \na.  Increasing the volume of the reaction vessel will reduce the pressure, favoring the production of more gaseous products, so the equilibrium will go to the right\nb.  Equal number of moles of gas on both sides, so increasing the volume will have no effect.\n\n1.  \na.  Decreasing the volume increases the pressure, favoring the side with fewer moles of gas.  Equilibrium would go to the left.\nb.  Equilibrium would go to the left, as there are fewer moles of gas on that side.
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CH3CONH2 + Na+-OH ---->  CH3COO -Na+ +  :NH3\n\nThis is a amide hydrolysis reaction, similar to the hydrolysis of an ester. Hydroxide attacks carbonyl to give tetrahedral intermediate. Explulsion of an amide ion gives a carboxylic acid, which is deprotonated quickly to give the carboxylate ion and ammonia.
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Here is one example ,\n\nAgNO3(aq) + NaCl(aq)-> AgCl(s)white precipitate + NaNO3(aq)
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Here's are a few:\nhttp://www.science-house.org/learn/CountertopChem/exp25.html\nhttp://www.chymist.com/copper%20silver%20gold%20expl.pdf\nhttp://chemlearn.chem.indiana.edu/demos/15-7%20TheGold1.htm
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It's [Cu(NH3)6]2+ or hexaamine copper (II)