When you reach that point you have not copied the complete equation. What you have is
K = 4.2E-6 = 4X^3/(0.07-2x)^2.
When I expand the denominator I obtained
4.2E-6 = 4X^3/0.0049-0.14x + 4X^2
To proceed you "cross multiply" and get
4.2E-6 * (0.0049 - 0.14x + 4X^2) = 4X^3
Then solve for X.
By the way, I applaud your reasoning for a and b and c.
A chemical system within a sealed 1 L reaction vessel is described by the following reversible reaction equation:
2H2S(g) <---> 2H(g) + S2(g)
If the equilibrium constant is 0.000 004 200 at 1103 K find:
(a) the reaction quotient intially
(b) the order of concentration of all three components at equilibrium without using calculations (From Greatest to lowest concentration)
(c) what the size of the reaction quotient indicates regarding the extent of the forward reaction
(d) the quilibrium concentration of sulphur gas if 0.070 mol of hydrogen sulphide gas is intially placed in the vessel
How I did a) was that I know that the equation for the reaction quotient was products/reactants. In this situation however, since I already have 0 moles of both products it would immediately mean that any number divided by 0 is 0.
For b) since I know that the Keq is a very small number, then that must mean that the reactants must also be a very small number. Next since it takes 2 moles of hydrogen gas for each sulfur gas, that tells me that the greatest is H2 then S2 then H2S
For c) Since I know the reaction quotient is 0 then that means that the forward reaction is very minimal or even close to not occurring.
Secondly:
For d)..... the Keq expression is [H2]^2[S2]/[H2S]^2 correct?
However, when I reach the part 4x^3/0.0049-0.28x+4x^2 I am stuck. Any help would be appreciated.
2 answers
the previous answer is correct up to the second point about expanding the denominator where the second coefficient should be -0.28?
1 answer