[Samlxo]

2NO_(g) + Cl_(g)  2NOCl_(g)

At 25°C, the total mixture of the three gasses in equilibrium is 1.55 atm. The percentage of the NOCL in the mixture is 77.4%. The mol fraction of the NO is 0.032. Calculate the K_c for the reaction.

So, I assume I would first express myself ... K_c=[NOCl]²/[NO]²[Cl₂]

Next I believe you make an "ICE" table

[NO]²_i:
[Cl₂]_i:
[NOCl]²_i:

[NO]²_eq:
[Cl₂]_eq:
[NOCl]²_eq:

Now I just can't seem to figure out how to use the percentage and mol fraction to come up with an answer.

I would imagine that the mol fraction formula, χ_a=mol A/mol total, as well as the mass percent formula, g A/ g total * 100, would play a roll. Also, would K_c be switched to K_p and the square brackets be changed to parentheses due to the pressure?

[Borek]

Knowing percentage of NOCl and mole fraction of NO should be enough to calculate amount of Cl₂ in the mixture. No need for ICE table.

[Samlxo]

Knowing percentage of NOCl and mole fraction of NO should be enough to calculate amount of Cl₂ in the mixture. No need for ICE table.

How would I use that data to get an answer?

Would I sub 0.032 in for X_a and use 2/x? So X_a=mol A/mol total :rarrow:0.032=2/x ?

But what would I do with the percentage of NOCl?

[Borek]

What is sum of molar fractions?

How is percentage related to molar fraction?

Note: for me question is unclear, as it doesn't say if it is a molar percentage, or mass percentage; problem looks solvable in both cases, but the result is different.