Question

@Kainui

Answer 1

@No.name Hey. =P

Answer 2

A 10.0 g sample of a mixture of calcium chloride and sodium chloride is treated with Na2CO3 solution. This calcium carbonate is heated to convert all the calcium to calcium oxide and the final mass of calcium oxide is 1.62 gm. The percentage by mass of calcium chloride in the original mixture is :

Answer 3

I don't want you to help me with this , actually just tell me what will be the reaction

Answer 4

Actaually i have the reaction but i don't know why is it

Answer 5

Is there a part of the reaction that's confusing in particular?

Answer 6

Yeah , the question is easy thouh

Answer 7

So the unbalanced equation is this: \[\LARGE NaCl + CaCl_2 +Na_2CO_3 \rightarrow CaO\] correct? How do we know that NaCl and CaCl2 are what these molecules look like? We can consult the periodic table and see that Ca is in the second column and Cl is in the 7th column meaning that Ca will likely lose 2 electrons while Cl will gain 2 electrons, allowing them to for CaCl2 to neutralize their charges. Similarly this is the case for others.

I'm not sure if that's what you're looking for or what?

Answer 8

The reactiopn written is
Cacl2 + Na2CO3 ---> CaCO3 +2Nacl

Answer 9

Oh I see, I wasn't thinking.

I was somehow thinking that CaO was directly formed but it's not. Also, where does the Sodium end up? If I had balanced it I would have noticed right away that something wasn't right.

So what happens first is that NaCl doesn't participate in the raction of CaCl2 with Na2CO3. Suppose it did, what will happen in the reaction of NaCl + Na2CO3? You wouldn't notice anything because the cations are the same.

Then afterwards what happens if we're then taking this CaCO3 and turning it into CaO.

Does that clear it up or did I leave something out? I'm sorta tired but I'll help you get through this one haha. =)

Answer 10

So that's why we did not include Nacl +Na2Co3 , because they won't react right?

Answer 11

Well to say they won't react is right for the most part. But likely these are dissolved into solution and you don't actually have either of these as separate entities, just 3Na+, 1Cl-, and 1CO3(2-).

Another thing to note is that chemical reactions are considered to be in "dynamic equilibrium" which means that in reality there is still a reaction going on, it's just that the rate of the forward reaction is equal to the rate of the backwards reaction so there is no net change in the total number of product and reactants.

Answer 12

that's what i was thinking , the textbook did not include them because they won't react