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Simple Stoic Qustion.........

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bucket:
I am back to annoy you guys with yet another question...

A solution containing 10.0g of silver nitrate is mixed with a solution containing 10.0g of barium chloride.
What mass of silver chloride precipitate is likely to be produced?
2AgNO3(aq) + BaCl2(aq) → 2AgCl(s) + Ba(NO3)2(aq)

The answers tell me its 8.44g

Thanks for any help in advance.

cara.mel:
*races to answer*

Again, these questions are testing you on limiting reagants.
n(AgNO3) = m/Mr = 10/169.9 = 0.0588mol
n(BaCl2) = m/Mr = 10/208.3 = 0.0480mol
AgNO3 is the limiting reagant as when all of it is used, you use 0.0294mol of BaCL2

=> n(AgCl) = 0.0588
m(AgCl) = n*Mr = 0.0588 * 143.4 = 8.44g

lanvins:

--- Quote from: kido_1 on January 30, 2008, 06:06:40 am ---Be careful with limiting reagants and determining mole ratios.


--- End quote ---

For my question, how do u noe whether u should use limiting reagants or mole ratios? Because if i use mole ratio than  Zn(S) and H2(g) are the same aren't they?

Collin Li:
You always use limiting reagents first (to figure out how many moles of reaction occurs), then you use mole ratios.

Even though , what is more important is that because it is limited by how much HCl there is in the first place.

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