- #1
reedy
- 37
- 0
Assignments given to me are drawn up in this manor:
There is 1,34 mol of X, 1,69 mol of Y and 1,95 mol of Z at equilibrium.
Calculate the equilibrium constant for the following reaction: [tex]2X + Y_2 \rightleftharpoons 2XY[/tex]
or sometimes the coefficients are left out in the equilbrium equation.
What I'm trying to say is that the coefficients are never the same as the number of moles given in the assignment.
I want to use
[tex]cC + dD \rightleftharpoons aA + bB[/tex]
[tex]K=\frac{[A]^a ^b}{[C]^c[D]^d}[/tex]
Should I use the coefficient in the equation or the exact number of moles from the assignment?
There is 1,34 mol of X, 1,69 mol of Y and 1,95 mol of Z at equilibrium.
Calculate the equilibrium constant for the following reaction: [tex]2X + Y_2 \rightleftharpoons 2XY[/tex]
or sometimes the coefficients are left out in the equilbrium equation.
What I'm trying to say is that the coefficients are never the same as the number of moles given in the assignment.
I want to use
[tex]cC + dD \rightleftharpoons aA + bB[/tex]
[tex]K=\frac{[A]^a ^b}{[C]^c[D]^d}[/tex]
Should I use the coefficient in the equation or the exact number of moles from the assignment?