Question

What are the final #of moles (theoretical ) out of 1.76g of cuco3 to cuo +co2?

Answer 1

For `CuCO_3(s) + Delta rarr CuO(s) + CO_2(g)`

Explanation:

We address the stoichiometric equation as written...

`underbrace(CuCO_3(s))_(123.56 *g)+ Delta rarr underbrace(CuO(s) + CO_2(g))_(123.56*g)`

And, as always, both CHARGE and MASS are conserved in EVERY chemical reaction....

In the given scenario, with respect to copper carbonate, we gots a molar quantity of `(1.76*g)/(123.56*g*mol^-1)=0.0142*mol`.

And, therefore, there must be molar quantities of `0.0142*mol` with respect to BOTH `"cupric oxide"`, and `"carbon dioxide...."`, which are the products of the reaction.

And so a mass of .............

`CuO(s)=0.0142*molxx79.54*g*mol^-1=1.13*g`.

And.....

`CO_2(g)=0.0142*molxx44.01*g*mol^-1=0.63*g`.

And does this represent the principle of conservation of mass? Why?

For transition metal carbonates, you have to heat the salt up very fiercely and thoroughly indeed to get all the carbon dioxide off....