2H2(g) + S2(g) ¡ê 2H2S(g)
Analysis of the contents of a 15.0L flask reveals that there are 4.4 moles of hydrogen gas, 2.0 moles of sulfur gas, and 3.7 moles of hydrogen sulfide gas in the flask at equilibrium. Calculate the equilibrium constant K
M each = mols/L = ?
Substitute M of each into the Keq expression for H2 + S2 ==> 2H2S and solve for Keq.
i got an answer of 39.776 because i did [mol/L H2S]^2/ [mol/L H2]^2[mol/L S2]^2 so im not sure what went wrong
What numbers did you substitute for concns H2, S2, H2S?
That should be (H2) = 4.4/15 = ?
(S2) = 2/15 = ?
(H2S) = 3.7/15 = ?
I suspect that's the problem.
i used those exact numbers
And your answers were?
after squaring i ended up with 0.060844444/ (1.529679004 *10^(-3)) = 39.7759555
What numbers do you get for
4.4/15 = ?
2/15 = ?
3.7/15 = ?
4.4/15= 0.293333333
2/15= 0.133333333
3.7/15= 0.246666666
So K = (0.24666)^2/(0.2933)(0.1333) =
Punch in the top numbers and divide by the bottom numbers WITHOUT copying any numbers; i.e., leave everything in the calculatord come up with an answer. I don't get 39.