Question

A(g) + B (g) ↔ C (g) + D (g)

Suppose that the concentrations of these gases in an equilibrium mixture were

[A] = 0.5 M
[B] = 4.0 M
[C] = 6.0 M
[D] = 8.0 M

How many moles of C would have to be added to the mixture to raise the equilibrium concentration of A to 1.0 M?

Answer 1

@Lena772 I feel that for this problem you could set it up and find what the Kc value is because you're given the equilibrium concentrations.

\[Kp = \frac{[C][D] }{ [A][B] }\]

Answer 2

48/2
Kp=24

Answer 3

let's think about this more, we are being told that we need to raise the concentration of A

Answer 4

clearly this value for Kp since it's greater than 1 suggests that the equilibrium favors the products.

Answer 5

yes should i do an ICE table?

Answer 6

yes I think so

Answer 7

My thoughts are that you would need to do an ice table, because in order for the concentration of A to increase Q > K and the equilibrium would have to shift to favor the reactants

Answer 8

BTW where did you get this question from it's very thought provoking

Answer 9

Chem21labs.com is the platform where all my G. Chem II course homework is. @Photon336