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What is the relationship between the concentration of sulfuric acid and the rate of reaction of

$$\ce{H2SO4(aq) + CaCO3(s) ⟶ H2O(l) + CO2(g) + CaSO4(aq)}$$

in the rate law:

$$\mathrm{rate} = k[\ce{H2SO4}]^n[\ce{CaCO3}]^m$$

So, if I were to change the initial concentration of sulfuric acid in the reaction how would the rate of formation of $\ce{CO2}$ change/the $\mathrm{pH}$ of the solution change?

Just looking for the order of the reaction in terms of the acid and perhaps a mechanism that might support this. I tried to make my own mechanism, but it seems to be nonsense so any help would be appreciated.

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  • $\begingroup$ Premise here is flawed. Even if reaction would be with, say, Na2CO3 dissolved in water in would it would be conc. of H+ to be considered. However it's a reaction with solid and for them there's no such thing as order of reaction at all! $\endgroup$ – Mithoron Nov 9 '19 at 20:46

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