Assorted Chem questions

[synchronise3]

The equilibrium constant is 10^–10 at 25°C for the reaction
Sn4+(aq) + 2Fe2+(aq) ----> Sn2+(aq) + 2Fe3+(aq)   (supposed to be double arrow)


Determine the value of the equilibrium constant for the reaction:
Sn2+(aq) + 2Fe3+(aq) -----> Sn4+(aq) + 2Fe2+(aq)   (supposed to be double arrow)

How would I go about solving this?

[afeichuu]

I might be wrong, but isn't it just the reciprocal of 10^-10, since the reaction if flipped?

[ligands]

I might be wrong, but isn't it just the reciprocal of 10^-10, since the reaction if flipped?

This is correct it will be for the equilibrium constant of the reverse reaction

[synchronise3]

I might be wrong, but isn't it just the reciprocal of 10^-10, since the reaction if flipped?

ah I see, lol didnt notice the reaction was flipped.
Thanks

[synchronise3]

Another Question,

Carbon monoxide is used as a fuel in many industries. It reacts according to the equation:
2CO(g) + O2(g) ---> 2CO2(g)   (supposed to be double arrow)
In a study of this exothermic reaction, an equilibrium system is established in a closed vessel of constant volume at 1000°C.

What will happen to the equilibrium constant as a result of the addition of more oxygen?

[charmanderp]

There wouldn't be any effect on the equilibrium constant, as only a change in temperature will affect that.

[synchronise3]

There wouldn't be any effect on the equilibrium constant, as only a change in temperature will affect that.

I can see how the change in temperature would affect it, but wouldn't the increase in oxygen cause a net forward reaction to counteract the effect of the additional oxygen?

And this would decrease the oxygen conc. while increasing the CO2 conc. ?

[Starlight]

Another Question,

Carbon monoxide is used as a fuel in many industries. It reacts according to the equation:
2CO(g) + O2(g) ---> 2CO2(g)   (supposed to be double arrow)
In a study of this exothermic reaction, an equilibrium system is established in a closed vessel of constant volume at 1000°C.

What will happen to the equilibrium constant as a result of the addition of more oxygen?

Wouldn't it drive the reaction to the right? (according to my lecture notes)

[charmanderp]

There wouldn't be any effect on the equilibrium constant, as only a change in temperature will affect that.

I can see how the change in temperature would affect it, but wouldn't the increase in oxygen cause a net forward reaction to counteract the effect of the additional oxygen?

And this would decrease the oxygen conc. while increasing the CO2 conc. ?

There's no net change in the concentration of any species though, it's just being stabilised.

[synchronise3]

Still kinda confused Doesn't the addition of oxygen cause an increase in concentration?

[charmanderp]

Yes but according to Le Chatellier's principle the system will react to neutralise the change ie. decrease the concentration of oxygen by pushing the reaction forward until a new equilibrium is reached.

[Tonychet2]

wouldnt the answer just be 10^-10?