Consider the reaction N2(g) + O2(g) 2NO(g), for which Kc = 0.10 at 2,000ºC. Starting with initial concentrations of 0.040 M N2 and 0.040 M O2, determine the equilibrium concentration of NO.
a) 5.4 × 10–3 M
b) 0.0096 M
c) 0.011 M
d) 0.080 M
e) 0.10 M
okay I keep getting 0.013 which isnt even on here, maybe im doing a significant digit error, and its C?
I set the problem up like this [NO]^2/[N2][O2]=.10
I know N2 and O2 are .040 so multiply .040 with .040 = .0016, multiple .0016 with .10 to get rid fo the denominator so the problem is now. [NO]^2 = .00016 take the square of both sides to get the concentration of NO = 0.0126 = 0.013 M??
2006-09-24
17:05:05
·
2 answers
·
asked by
hmmm
2
in
Chemistry