posted by Julia
please help and explain.
At a certain temperature, Keq = 10.5 for the equilibrium below.
CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g)
Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing 1.01 mol/L CO and 0.335 mol/L CH3OH
At 2273 K, Keq = 6.2 multiplied by 10-4 for the following reaction.
N2(g) + O2(g) equilibrium reaction arrow 2 NO(g)
If [N2] = 0.04700 mol/L and [O2] = 0.01200 mol/L, what is the concentration of NO at equilibrium?
please answer and explain this one as well.
CO(g) + 2 H2(g) <==> CH3OH(g)
Keq = 10.5 = (CH3OH)/(CO)(H2)^2
You know K, (CH3OH), and (CO). Substitute and solve for (H2)
For the N2 + O2 ==> 2NO problem, is 0.04700 M and 0.01200 M the concentrations at the beginning of the reaction and you want to find the equilibrum concns for NO OR are those concns those at equilibrium and you want to find the equilibrium concn of NO?
Idk google it