# HARD Half Equation

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#1
cl2+ naoh --> naclo3 + nacl +h20. I'm really struggling to do the half equation for this ;(. I know it's a disportionation reaction and i know the oxidation states of everything. It's just i got it wrong ;( PLZ help!
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#2
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4 years ago
#3
You mean the ionic equation?

Na+ + Cl- ==> NaCl all aqueous.
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#4
(Original post by Xenon17)
You mean the ionic equation?

Na+ + Cl- ==> NaCl all aqueous.
n0 but how did u get the ionic eq anyhow
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4 years ago
#5
n0 but how did u get the ionic eq anyhow
For ionic equations, look at the product which is formed which is Nacl in this case, and form an equation using just the ions involved. Here, it will be the Na and Cl ions.

Na has a 1+ charge, and Cl has a 1- charge so they are aready balanced in terms of charges. So, we just form the equation:

Na+ + Cl- --> NaCl

For example now if the product was MgCl, then you would need 2 Cl ions as the Mg is a 2+ ions and you need to balance the charges:

Mg2+ + 2Cl- --> MgCl

For the half equation, what is the questions asking you to form the half equation for and from what? I'll go through it with you 0
#6
(Original post by derpz)
For ionic equations, look at the product which is formed which is Nacl in this case, and form an equation using just the ions involved. Here, it will be the Na and Cl ions.

Na has a 1+ charge, and Cl has a 1- charge so they are aready balanced in terms of charges. So, we just form the equation:

Na+ + Cl- --> NaCl

For example now if the product was MgCl, then you would need 2 Cl ions as the Mg is a 2+ ions and you need to balance the charges:

Mg2+ + 2Cl- --> MgCl

For the half equation, what is the questions asking you to form the half equation for and from what? I'll go through it with you that topic question half equation 0
4 years ago
#7
Moved to chemistry.
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4 years ago
#8
Consider each of the chlorine atoms separately

1) 1/2 Cl2 + e- ----> Cl-

2) The second one ends up in the chlorate ion - ClO3-

1/2 Cl2 ----> ClO3-

How would you go about balancing the second?

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#9
(Original post by Serine Soul)
Consider each of the chlorine atoms separately

1) 1/2 Cl2 + e- ----> Cl-

2) The second one ends up in the chlorate ion - ClO3-

1/2 Cl2 ----> ClO3-

How would you go about balancing the second?

how chlorate ions this is what i wasn't getting ;(
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4 years ago
#10
how chlorate ions this is what i wasn't getting ;(

When we're doing simpler half equations, we usually have some oxygen atoms involved don't we?
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4 years ago
#11
cl2+ naoh --> naclo3 + nacl +h20. I'm really struggling to do the half equation for this ;(. I know it's a disportionation reaction and i know the oxidation states of everything. It's just i got it wrong ;( PLZ help!
Do really mean half equation or are you just trying to balance this?

3Cl2 + 6NaOH ---> NaClO3 + 5NaCl + 3H2O
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#12
(Original post by TeachChemistry)
Do really mean half equation or are you just trying to balance this?

Cl2 + 6NaOH ---> NaClO3 + 5NaCl + 3H2O
HALF equations
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#13
(Original post by Serine Soul)

When we're doing simpler half equations, we usually have some oxygen atoms involved don't we?
normally if its a compound we don't split it up in half equations can u split up ionic compound only I'm not sure .

cause in MgO +Cu --> Mg + CuO

we say half eq is: mg2+ +2e--> mg

and cu --> cu2+ +2e-

but there there are half equations like mno3- --> mn

we say Mno3- +5e- +6h+ --> mn + 3h20 (we added water and h+ to balance the charge and atoms).

but like i split the compound at the top why can't we do the same and say

mn+5 +e- --> mn, like we did with magnesium I'm really confused on this part cause originally for naclo3 i just try to add that in the half equation but you split it up ? why and how do you know that clo3- forms a ion, why cudnt it not be 3/2o2- + cl-1?? i have this gap in my knowledge and i keep messing things up plz help
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4 years ago
#14
HALF equations
O.5Cl2 + 6OH- --> ClO3- + 3H2O + 5e-
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#15
(Original post by TeachChemistry)
O.5Cl2 + 6OH- --> ClO3- + 3H2O + 5e-
how ? you got that
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4 years ago
#16
how ? you got that

You gave chlorate (V) in the original post so I just wrote the half equation for chlorine to that.
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#17
(Original post by TeachChemistry)
You gave chlorate (V) in the original post so I just wrote the half equation for chlorine to that.
how do u know when to split up chlorate? cause some formulae like Mno3- u don't split up,like how do u know what ions are formed is there something i gotta learn ;(
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4 years ago
#18
how do u know when to split up chlorate? cause some formulae like Mno3- u don't split up,like how do u know what ions are formed is there something i gotta learn ;(
I do not understand what you have written here. You were the one who provide initial equation. I just broke it down into half equations like you asked.
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