[cho_reunited]

1) Gas X₂ reacts with gas Y₂ to give gaseous XY according to this equation:
X₂ + Y₂ <=> 2XY
The equilibrium constant for the reaction is found to be 2.6 x 10^-3
What will be the value of K_eq for the reverse reaction?

The answer is 3.8 x 10²
but I have no clue how they got that.



2) The equilibrium constant for the reaction A + B <=> C + D is 7.0 x 10⁵
At a non-equilibrium situation, [A] = 0.4M, the molarity of B = 0.4M, [C] = 0.8M, [D] = 0.2M
Assuming sufficient activation energy, why does the would the reaction shift to the right (products) ?

[cho_reunited]

3) When initial concentrations of SO₂ = 1.62M and 0₂ = 0.82M are heated, an equilibrium is established in which [SO3] = 1.22M.
If the equation is 2SO_{2 (g)} + O_{2 (g)} <=> 2SO_{3 (g)} then what will be the value of K_eq?

the answer is 44 but I haven't the foggiest how to get that.

[cho_reunited]

4)   The thermal dissociation of calcium carbonate is as follows:
CaCO_{3 (s)} + heat <=> CaO _(s) + CO_{2 (g)}
In describing the compositions of different equilibrium mixtures produced at the same temperature by the above reaction, it is correct to say that all compositions have the same partial pressure of CO₂
^^why is this?

[sjb]

1) Gas X₂ reacts with gas Y₂ to give gaseous XY according to this equation:
X₂ + Y₂ <=> 2XY
The equilibrium constant for the reaction is found to be 2.6 x 10^-3
What will be the value of K_eq for the reverse reaction?

The answer is 3.8 x 10²
but I have no clue how they got that.

What is the expression for the equilibrium constant for the forward, and reverse reactions?

2) The equilibrium constant for the reaction A + B <=> C + D is 7.0 x 10⁵
At a non-equilibrium situation, [A] = 0.4M, the molarity of B = 0.4M, [C] = 0.8M, [D] = 0.2M
Assuming sufficient activation energy, why does the would the reaction shift to the right (products) ?

What is the expression for the equilibrium constant?

[cho_reunited]

I don't know, that information isn't given to me.

[Borek]

You should know how to write these expressions, they are the most basic thing in the equilibrium calculation. They are not given - but you can write them just after seeing reaction equation.

[cho_reunited]

I do know how to write expressions...but that doesn't help me here.

[Borek]

Try to multiply K_forward*K_reverse. What do you get?

[Vidya]

K  reverse  reaction =1/ K forward