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You carefully weigh out 18.00g of CaCO3 powder and add it to 72.90 g of HCl solution. You notice bubbles as a reaction takes place. You then weigh the resulting solution and find that it has a mass of 83.52g. The relevant equation is

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

Assuming no other reactions take place, what mass of CO2 was produced in this reaction?

Respuesta :

For the reaction CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) the mass of CO2 will be 7.38 grams.

What is CO2?

CO2 is a type of gas which is the combination of one atom of carbon and two atom of oxygen they as bonded with each other with covalent bond.

In the reaction  CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq) CO2 will pass away in the form of gas as to total expected mass is 90.9 gram but the mass is 83.52 so, the carbon remain is 7.38 grams after subtracting.

Therefore,  the mass of CO2 will be 7.38 grams the reaction CaCO3(s)+2HCl(aq)→H2O(l)+CO2(g)+CaCl2(aq)

Learn more about CO2, here:

https://brainly.com/question/11639748

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