[uxk8396]

CaCO3(s)+2HCl(aq)⟶H2O(l)+CO2(g)+CaCl2(aq)

(i) From the above equation, if the volume of water increases, does the rate of reaction also increase? Please explain.
 
(ii) Will the pressure of the carbon dioxide gas increase, if water is increased?

How do we essentially approach to solve these types of questions?
Thanks

[uxk8396]

CaCO3(s)+2HCl(aq)⟶H2O(l)+CO2(g)+CaCl2(aq)

Not sure if there is an edit button, however, I have re-phrased the question:

1) If water is added into the conical flask in the above experiment, how will this affect the rate of reaction?

2) And if the pressure of the carbon dioxide gas increase, will this speed up the reaction?

[docnet]

I think the forum rules state that you have to make an attempt at answering the questions before we can help you. What do you think about the effect of the solution's volume increase?

What affects the rate of a chemical reaction?

[AWK]

This is (practically) non-equilibrium reaction. But some other equilibria will exist depending on amount of HCl (limiting reagent, stoichiometric amount or excess of HCl)

[uxk8396]

I presume that the reaction rate will also increase because as the water increases in the conical flask, there is less space for the carbon dioxide gas molecules which would increase the pressure exerted on the inside wall of the container. I referred to the Ideal Gas Law's theory (PV=nRT)

Kindly advise if I am guessing that correctly. Thanks

[AWK]

Which stoichiometry of reaction (from 4 possible) do you mean? Remember that carbon dioxide is relatively well soluble in water and another equilibrium CO₂(aq)-CO₂(g) exists if carbon dioxide is evolved at all. You should know real data to discuss these quite complex equlibriums.