2HCl (aq)+CaCO3 (s)->H20(l)+CaCl2(aq)+CO2(g). If using 40cm^3 of 2.5mol.dm^-3 Hcl and 5.67g of CaCO3, determine the limiting reagent and how much CO2(g) could be theoretically produced by this reaction.

First, we have to convert the starting measurements for the HCl and CaCO3 content into moles so we can compare the ratios to the formula. 40cm^3=0.04dm^30.04dm^32.5mol.dm^-3=0.1 moles of HClmass/molar mass= moles5.67g/100=0.0567 moles of CaCO30.1 moles of HCl will fully react to 0.05 moles of CaCO30.0567>0.05 so HCl is the limiting reagent 0.1 moles of HCl fully reacting will produce 0.05 moles of CO2 as the coefficient of HCl is 2 and the coefficient of CO2 is 1.0.05 moles CO244 g/mol=2.2 grams of CO2(g)

DR
Answered by Daniel R. Chemistry tutor

2375 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

Explain why average bond enthalpies can be used for cyclohexane but not for benzene


Why is there a significant difference between the radii of first and second row transition metals, where as no difference (or even a decrease) is observed between the second and third rows?


Sodium and sodium iodide can both conduct electricity when molten, but only sodium can conduct electricity when solid. Explain this difference in conductivity in terms of the structures of sodium and sodium iodide.


Calculate: (a) The amount, in mol, of white phosphorus used, (b) the limiting reagent, (c) the excess amount, in mol, of the other reagent.


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning