Equilibrium Constant Calculation (simple one) - please check my working out :)

At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

Get our expert's

answer on brainly

SEE EXPERT ANSWER

Get your free account and access expert answers to this and thousands of other questions.

A community for students.

Equilibrium Constant Calculation (simple one) - please check my working out :)

Chemistry
See more answers at brainly.com
At vero eos et accusamus et iusto odio dignissimos ducimus qui blanditiis praesentium voluptatum deleniti atque corrupti quos dolores et quas molestias excepturi sint occaecati cupiditate non provident, similique sunt in culpa qui officia deserunt mollitia animi, id est laborum et dolorum fuga. Et harum quidem rerum facilis est et expedita distinctio. Nam libero tempore, cum soluta nobis est eligendi optio cumque nihil impedit quo minus id quod maxime placeat facere possimus, omnis voluptas assumenda est, omnis dolor repellendus. Itaque earum rerum hic tenetur a sapiente delectus, ut aut reiciendis voluptatibus maiores alias consequatur aut perferendis doloribus asperiores repellat.

Get this expert

answer on brainly

SEE EXPERT ANSWER

Get your free account and access expert answers to this and thousands of other questions

Where's the calculation?
oops sorry, internet cut out. Here it is: In a laboratory test of this equilibrium 6.00 mole of SO2 and 2.50 mole of O2 are added to 2.00L reaction vessel and allowed to come to equilibrium at 700 degrees celsius. If 4.00 mole of SO3 is present at equilibrium, what is the value of the equilibrium constant? \[2SO_2 (g) + O_2 (g) <=> 2SO_3 (g)\] So, i drew up an ICE table. |dw:1436876239363:dw| divide by 2 to obtain concentration: |dw:1436876365753:dw| So then the K constant: \[K_c = \frac{ [SO_3]^2 }{ [SO_2]^2 \times [O_2]}\] \[K_c = \frac{ [2.00]^2 }{ [1.00]^2 \times [0.25] } = 16\] I feel like i'm also meant to refer to the temperature (700 degrees celsius) but i'm not too sure? :/
The equation doesn't include temperature but it's implied from the value of the equilibrium constant for the reaction, because that will change depending on your temperature.

Not the answer you are looking for?

Search for more explanations.

Ask your own question

Other answers:

I got something around 16 for Kc but I think you need to consider converting to Kp because this is a gaseous reaction since Partial pressures apply.
1 Attachment
There's a formula to convert Kc to Kp and for this you need the temperature. Kp = Kc (RT)^( delta n) Delta n = #moles of gas of product - #moles reactants. R = 0.08 L mol^-1 atm K^-1 T = K
oh interesting. I haven't learnt about partial pressures yet, but i'll note it down just in case :) thanks.
Yeah, so for that; the partial pressure In a sealed container the pressure is equal to the sum of the pressures exerted by each individual gas. Which is the mole fraction of that gas multiplied by the total pressure. So if we had a sealed container at some pressure with say two gases A and B one was 2 moles while the other 4; it would be 6 mole of gas total Gas A 2/6 Gas B. 4/6 So pressure total = 2/6*Ptotal+4/6*Ptotal.
thank you again!! :D

Not the answer you are looking for?

Search for more explanations.

Ask your own question