This is not a decomposition reaction.
2H2,g + O2,g --> H2Ol
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The reaction is: CaO(s) + H2O(l)--- --> Ca(OH)2(s) Ca(OH)2(s) is the product (at the right side of the reaction equation).
If you added less than the amount needed in part (b) of K2SO3, what would be the limiting reactant? If you added more than the amount needed in part (b) of K2SO3, what would be the limiting reactant? Which situation would create the most SO2 gas?excess HClexcess K2SO3 excess H2Oexcess KClperfectly matched amounts of HCl and K2SO3
Just set up the balanced equation to solve this. C3H6 (s) + (9/2)O2(g) ---> 3CO2(g) + 3H2O (l). Now it is only a matter of adding and subtracting the appropriate formation values.
2H2,g + O2,g --> H2Ol
It means that it is in a liquid state as opposed to solid (ice) or gas (water vapour or steam)
Melting
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If it's in the form H2O(l) then the l stands for liquid. This is to show that liquid water is different than gaseous water (steam), which would be H2O(g) with a g for gas.
The reaction is: CaO(s) + H2O(l)--- --> Ca(OH)2(s) Ca(OH)2(s) is the product (at the right side of the reaction equation).
It dissolves and forms carbonic acid, by: CO2,g + H2Ol --> H2CO3,aq , a very weak diprotic acid.
6.6 x 10-9
2NaOHaq + 2HClaq --> 2NaClaq + H2Ol is the perfect balanced equatiion,except the solubility (aq) of NaCl, so it is notNaCls but NaClaq
6.6 x 10-9
Balanced Molecular Equation: CaO(aq)+2HCl(aq) --> CaCl2 (aq) + H2O(l) Balanced Total Ionic Equation: Ca(aq)+2 + O(aq)-2 +2H(aq)+ + 2Cl(aq)-2 --> Ca(aq)+2 + 2Cl(aq)-2 + H2O(l) Total Ionic Equation: O(aq)-2 +2H(aq)+ --> H2O(l)