BaCO3 + 2HNO3 ==> Ba(NO)3)2 + H2CO3 and
H2CO3 ==> H2O + CO2.
CO3^2-(aq) + 2H^+(aq) ==> H2O(l) + CO2(g) is the net ionic equation.
#1 makes no sense. Ba(NO3)2 is a PRODUCT, not a reactant.
#2.
BaCO3 + 2HNO3 ==> Ba(NO3)2 _+ H2O + CO2
mols BaCO3 = M x L = about 0.00375 but you should confirm that.
Convert mols BaCO3 to mols CO2
Then use PV = nRT. You know T, R, n, V, solve for P. Remember T must be in kelvin; P will be in atm if you use R = 0.08206.
Barium carbonate and nitric acid reacts in a double displacement reaction. One of products also dissociates and evolves carbon dioxide. Write the net ionic reaction including the proper use of phase labels for this solution run in aqueous solution.
After this the following questions ask:
1. For the reaction in problem 2, if 25.0 mLs of 0.150M nitric acid was used, how many grams of barium nitrate would be required for complete reaction?
2. For the reaction from problem 2, if 0.5000 grams of barium carbonate was reacted with 25.0mLs of 0.15M nitric acid and the ags then collected in 100mL flask at 77 degrees celsius, what is the gas pressure in the flask?
**I am struggling big time on these questions. Please help! Thank you so muchhh**
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