Quick Chemistry Question

2009-09-02 15:56:01

#1

Ryan: Member; +1,230|7263|Alberta, Canada

Ok, so I only have like 3 questions left on this review (I'm doing a review of grade 11 chem before we start the real chem 30 stuff) and I'm kinda confused.

The question reads:

Write the dissociation equation and calculate the concentration of each ion or solution.

1. 0.265mol/L iron (III) chloride

So I wrote the equation as

2FeCl_{3 (aq)} ------> 2Fe³⁺_(s) + 3Cl₂^-_(g)
0.265 mol/L c c
162.2 g/mol

I'm not given the volume of the iron (III) chloride, so how can I determine the number of moles of it?

I need to use c=nv to find concentration, but I don't have moles, or the volume of any of the substances...

Am I missing something or am I just dumb?

Last edited by Ryan (2009-09-02 15:57:07)

2009-09-02 15:59:07

#2

DesertFox-: The very model of a modern major general; +796|7104|United States of America

I'm a bit rusty myself but I think you can use the K_eq to find those concentrations if I'm not mistaken.

2009-09-02 15:59:30

#3

Ryan: Member; +1,230|7263|Alberta, Canada

... I don't think I've learned that yet.

2009-09-02 16:03:57

#4

menzo: ̏̏̏̏̏̏̏̏&#; +616|6866|Amsterdam‫

2FeCl3 (aq) ------> 2Fe3+(s) + 3Cl2-(g)
0.265 mol/L 0.265 mol/L 0.265 mol/L * 1.5 = 0.3875 mol/L

1 1 1.5 ratio

there the will be the ammount of 2FeCl3 (aq) and 2Fe3+(s )
and there is 1.5x as much Cl2

Last edited by menzo (2009-09-02 16:12:37)

https://i231.photobucket.com/albums/ee37/menzo2003/fredbf2.png

2009-09-02 16:20:53

#5

Ryan: Member; +1,230|7263|Alberta, Canada

Ah ok, thanks

2009-09-02 16:33:40

#6

Bevo: Nah; +718|6941|Austin, Texas

edit: I completely confused the shit out of myself.

Last edited by Bevo (2009-09-02 16:39:57)

2009-09-02 16:37:24

#7

menzo: ̏̏̏̏̏̏̏̏&#; +616|6866|Amsterdam‫

he needs concentration so mol/L
if you have the same amount of molecules before and after the reaction the concentration stays the same

Last edited by menzo (2009-09-02 16:38:15)

2009-09-02 16:41:26

#8

Bevo: Nah; +718|6941|Austin, Texas

menzo wrote:
he needs concentration so mol/L
if you have the same amount of molecules before and after the reaction the concentration stays the same

Yes, no you're correct. Sorry I just tried to make a very basic problem into something else. Excuse my chem spazm. I'm too used to doing confusing as shit problems.

2009-09-02 18:33:29

#9

S.Lythberg: Mastermind; +429|6866|Chicago, IL

you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-

2009-09-02 18:35:56

#10

Bevo: Nah; +718|6941|Austin, Texas

S.Lythberg wrote:
you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-

Way to make yourself look like a dumbass.

cl2, as in diatomic chlorine, the one that's a gas.

2009-09-02 18:37:13

#11

S.Lythberg: Mastermind; +429|6866|Chicago, IL

Bevo wrote:
S.Lythberg wrote:
you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-
Way to make yourself look like a dumbass.

cl2, as in diatomic chlorine, the one that's a gas.

he's wrong, it's not Cl2, it is a simple ion dissociation, into aqueous Cl-

2009-09-02 18:38:00

#12

justice: OctoPoster; +978|7161|OctoLand

S.Lythberg wrote:
Bevo wrote:
S.Lythberg wrote:
you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-
Way to make yourself look like a dumbass.

cl2, as in diatomic chlorine, the one that's a gas.
he's wrong, it's not Cl2, it is a simple ion dissociation, into aqueous Cl-

Agreed

I know fucking karate

2009-09-02 18:39:17

#13

Bevo: Nah; +718|6941|Austin, Texas

oh fuck, i thought that was the question.

ryan, you fail.

2009-09-02 18:41:37

#14

ceslayer23: IN YOUR MIRROR; +142|6781|CLOSER THAN I APPEAR

say the title of this post 5 times fast

2009-09-02 18:43:02

#15

Ryan: Member; +1,230|7263|Alberta, Canada

Bevo wrote:
S.Lythberg wrote:
you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-
Way to make yourself look like a dumbass.

cl2, as in diatomic chlorine, the one that's a gas.

Exactly, lol.

S.Lythberg wrote:
Bevo wrote:
S.Lythberg wrote:
you guys fail at chemistry

Iron (III) chloride dissociates into Fe 3+ and 3Cl-

if you have 0.265mol/L of FeCl3, it will dissociate into .265 mol/L Fe 3+ and .795 mol/L Cl-
Way to make yourself look like a dumbass.

cl2, as in diatomic chlorine, the one that's a gas.
he's wrong, it's not Cl2, it is a simple ion dissociation, into aqueous Cl-

Wait, what? Why? lol

If chlorine is by itself, it's diatomic, therefor Cl2.

Last edited by Ryan (2009-09-02 18:43:59)

2009-09-02 18:44:47

#16

Bevo: Nah; +718|6941|Austin, Texas

Dissociation means they're still aqueous.

Write the dissociation equation and calculate the concentration of each ion or solution.

1. 0.265mol/L iron (III) chloride

FeCl3 --> Fe3+ + 3Cl-

lyth was correct.

Last edited by Bevo (2009-09-02 18:46:31)

2009-09-02 18:45:55

#17

justice: OctoPoster; +978|7161|OctoLand

You need to go back and study the basics of dissociation Ryan, it will kill you in the exam.

Last edited by justice (2009-09-02 18:46:09)

I know fucking karate

2009-09-02 18:47:08

#18

S.Lythberg: Mastermind; +429|6866|Chicago, IL

Bevo wrote:
Dissociation means they're still aqueous.

Write the dissociation equation and calculate the concentration of each ion or solution.

1. 0.265mol/L iron (III) chloride

FeCl3 --> Fe3+ + Cl-

lyth was correct.

this

Cl- is more stable in solution than Cl2, which would evaporate (and clear out your sinuses quite nicely)

2009-09-02 18:47:14

#19

Ryan: Member; +1,230|7263|Alberta, Canada

justice wrote:
You need to go back and study the basics of dissociation Ryan, it will kill you in the exam.

We hardly covered it in chem 20, so no I do not.

I was always taught that all the halogens were diatomic, P4, S8, H2, N2, and O2.

2009-09-02 18:48:52

#20

Ryan: Member; +1,230|7263|Alberta, Canada

Well I looked it up, I guess you guys are right.

I was never taught that, I don't know how I'll ever remember to do that...

2009-09-02 18:51:18

#21

Bevo: Nah; +718|6941|Austin, Texas

they are diatomic in gaseous form. But they don't simply become diatomic again after dissociation. dissociation is the splitting of ions in a compound.

2009-09-02 18:51:31

#22

S.Lythberg: Mastermind; +429|6866|Chicago, IL

Ryan wrote:
justice wrote:
You need to go back and study the basics of dissociation Ryan, it will kill you in the exam.
We hardly covered it in chem 20, so no I do not.

I was always taught that all the halogens were diatomic, P4, S8, H2, N2, and O2.

none of those are halogens...

and only in the gaseous state, they become P(+/-)4, S-2, H+, NO3- (I've never seen free N, too unstable, N3- (azide) can exist for short periods), and O-2 in solution.

All halogens assume a -1 charge in solution, to complete their valence electron shell

Last edited by S.Lythberg (2009-09-02 18:52:01)

2009-09-02 18:52:31

#23

Bevo: Nah; +718|6941|Austin, Texas

NO2- too, and H3O+ (which is essentially H+)

the diatomic ones are HOBrFINCl

H2, O2, Br2, F2, I2, N2, Cl2

Last edited by Bevo (2009-09-02 18:53:49)

2009-09-02 18:53:27

#24

Ryan: Member; +1,230|7263|Alberta, Canada

S.Lythberg wrote:
Ryan wrote:
justice wrote:
You need to go back and study the basics of dissociation Ryan, it will kill you in the exam.
We hardly covered it in chem 20, so no I do not.

I was always taught that all the halogens were diatomic, P4, S8, H2, N2, and O2.
none of those are halogens...

and only in the gaseous state, they become P(+/-)4, S-2, H+, NO3- (I've never seen free N, too unstable, N3- (azide) can exist for short periods), and O-2 in solution.

All halogens assume a -1 charge in solution, to complete their valence electron shell

ugh, my god. The fucking halogens are or whatever, then theres phosphorus and oxygen and shit. Who cares?

2009-09-02 18:54:52

#25

S.Lythberg: Mastermind; +429|6866|Chicago, IL

Ryan wrote:
S.Lythberg wrote:
Ryan wrote:

We hardly covered it in chem 20, so no I do not.

I was always taught that all the halogens were diatomic, P4, S8, H2, N2, and O2.
none of those are halogens...

and only in the gaseous state, they become P(+/-)4, S-2, H+, NO3- (I've never seen free N, too unstable, N3- (azide) can exist for short periods), and O-2 in solution.

All halogens assume a -1 charge in solution, to complete their valence electron shell
ugh, my god. The fucking halogens are or whatever, then theres phosphorus and oxygen and shit. Who cares?

you should, oxygen and nitrogen are the bulk of earth's atmosphere, and responsible for most of the chemistry in your body.

Fluorine will melt your glasses

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