How Do You Balance the Reaction Between Nitric Acid and Calcium Carbonate?

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    Ap Chem Response
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The discussion focuses on predicting the balanced equation for the reaction between excess nitric acid and solid calcium carbonate. The initial attempt presented was H+ + CO3 → H2O + CO2, which was acknowledged as incomplete. The participant recognized the need to include calcium and nitrate ions for a complete equation. They also noted that the AP exam does not require spectator ions to be shown, clarifying their confusion stemmed from not indicating the 2+ charge for carbonate. Ultimately, the participant concluded that their equation was not balanced.
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Homework Statement


My questions pertain to #4b of the free response.

Question: Excess nitric acid is added to solid calcium carbonate. The question asks to predict a balanced equation for this reaction.




The Attempt at a Solution



what I wrote down was:

H+ + CO3 ----> H2O + CO2

which might be down the right road but isn't correct.
 
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What about bicarbonate?

Show the calcium as well as nitrate for completeness.
 
woops

I should have included that the AP exam does not require that you show spectator ions, I realized shortly after posting that my confusion was only coming from not writing in the 2+ charge for the carbonate, so I think that what I have is generally correct.
 
The equation is not balanced.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
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