If CO2 + H2O= H2CO3 would this reactin raise, lower, or have no effect on the water level?
464536
this is a very good question, i never thought of it this way.\n\nI think the level will increase but very small amount.\n\nCO2 is being added to the water and forming H2CO3, this is staying in solution. So nothing is lost, only CO2 is being added. The density will be a little higher now, so the volume will not change by much, but should be on the postive side.\n\nOnly about one mole of CO2 can be put into solution at room temperture, which isnt much. So any change in density and volume will be very small.\nWill take too much of my time to work out the excact numbers, but what a good question.
787481
NaHCO2 + H2SO4 --> Na2SO4 + CO2(g) + H2O(L)\n\nSodium bicarbonate + sulphuric acid equals sodium sulfate + carbon dioxide + water
433273
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.
696429
sodium ethanoate and carbon dioxide along with water
615100
the same elements except that \n-the ammount of CO2 inceases to 4%(not certain about the value)\n-the oxygen ammount decreeases to 16%\n-the water vapour ammount also increases
773341
No precipitate is formed.\nYou will see bubbles of carbon dioxide if there is enough HCI (Na2CO3+2HCI=2NaCI+H2O+CO2). If there isn't enough HCI ,Na2CO3+HCI=NaHCO3+NaCI happens ,you will see nothing.
843536
Calcium Carbonate (CaCO3) is insoluble, therefore it is the precipitate --> makes the solution cloudy.  The H2O is just plain old water. I believe the equation to which you are referring is H2CO3 + Ca(OH)2 --> CaCO3 +H2O, however, but no big deal.
785032
When CO2 dissolves in water it forms the weak acid carbonic acid. H2CO3. As temp of air increases the surface temp of the ocean will increase and the solubility of CO2 will increase
551370
Well, the equation is..\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2CO3 (Carbonic Acid) \n(or)\nCH3COOH + NaHCO3 ----> CH3COONa (Sodium Acetate) + H2O (Water) + CO2 (Carbon-dioxide)\n\nSo you might have noticed the equation is already balanced. It is a double-displacement reaction. So the sides are already balanced.\nHope this helps.\n\nOne small note...I don't think there is a compound such as NaCO3. The valency of CO3(^-2) ion is 2, so it has to combine with two Sodiums (two positive charges to neutralise its two negative charges) unless the compound one of the above users mentioned is NaCO3-.\n\nrule wid style n luv@vinny
441451
Well, there's a decomposition reaction.\n\nH2CO3 <--> H2O + CO2\n\nCarbonic acid (H2CO3) doesn't not exist much at all, because it decomposes into H2O and CO2. But some of the carbonic acid remains, pushing up the hydronium concentration, which by definition makes water more acidic. Therefore, getting rid of the CO2 in water makes water less acidic (raising the pH).
925123
if the water is at very very low pressure it can become gaseous.\n\nSee also - the triple point of water
744972
It's easy. Just remember that carbon dioxide can dissolve in water to form carbonic acid. i.e. CO2(gas) + H2O(aqueous) => H2CO3 (aqueous)
270274
ur equation is wrong....\nu will get H2O + C...\ncheck again\nif it's correct, u have to find out which one is the limiting reagent by calculating the number of moles of each reactant used...thus figuring out the number of moles of product and multiplying with the molecular mass of methanol...
804535
Neutralization Reaction:\nHC2H3O2(aq) + KOH(aq) -->H2O(l) + KC2H3O2(aq)\nThe equation is already balanced.\n\na. False KC2H3O2(aq) and H2O are products.\nb. True\nc. False, some ions will cancel out but some will remain.\n\nThe ionic equation is as follows:\n(H^+)(aq) + (C2H3O2^-)(aq) + (K^+)(aq) + (OH^-)(aq) -->H2O(l) + (K^+)(aq) + (C2H3O2^-)(aq)\nRepeated ions are crossed off from both sides and the net ionic equation is:\n(H^+)(aq) + (OH^-)(aq) -->H2O(l)\n\nd. True\ne. False\n\nNote: the + and - signs were written with ^ to indicate that they were raised up (like a power).  Sorry if this notation is confusing.  Good luck and I hope that this helps!
725776
Water under pressure (i.e. deep underground) can dissolve large amounts of CO2 if there is CO2 around then the water will become carbonated.
835769
After suitable corrections, yes.\n\nDecarboxylation liberates CO2 from the carboxyl group.\nIf your 'gas trap' is a graduated tube up which the CO2 can bubble, displacing water as it gathers at the top, its vol can be measured.\n\nHowever, two corrections must be made to this vol:\n1)The pressure and temperature of the CO2 must be measured, and the vol corrected to STP...Std Temp & Press\n2) CO2 is soluble in water to some extent...so you must determine the amount dissolved in the water...which can be done by titrating with a standardized base.\n\n2) is not necessary if CO2 is not soluble in the liquid used, eg.mercury.
887756
Basic balancing of chemical reactions. You can always add CO2 O2 and H2O to either side. Start with the Carbon. balance the Oxygen last since it is contained in CO2 and H2O.\n\n1) 2 C6H6 + 15 O2 ==> 12 CO2 + 6 H2O\n2) C12H22011 + 12 O2 ==> 12 CO2 + 11 H20\n3) C3H6O + 4 O2 ==> 3 CO2 + 3 H2O\n4) C4H10O + 6 O2 ==> 4 CO2 + 5 H2O\n5) C4H10O + 6 O2 ==> 4CO2 + 5 H2O