Post by: vamsiaus on July 18, 2009, 02:11:11 pm
A 2.00 mol sample of nitrosyl bromide, NOBr, was introduced into a 5.0 L vessel. At equilibrium, the concetration of nitrosyl bromide was found to be .0750 M. Calculate the equilibrium constant for the reaction shown in the equation:
2NOBr(g) (equilibrium Arrow) 2NO(g) + Br2 (g)
What I already did was to work out the equation to go ((1.625 ^2) x (.8125)) / (.375^2) which gives me 15.26, but the answer is 3 something. so just wondering if somebody can help me out with what i have done wrong. this question was part of a worksheet our teacher gave us as a preparation for the upcoming sac. So yeah Thanks to anybody who can help.
Post by: monokekie on July 18, 2009, 02:33:05 pm
A 2.00 mol sample of nitrosyl bromide, NOBr, was introduced into a 5.0 L vessel. At equilibrium, the concetration of nitrosyl bromide was found to be .0750 M. Calculate the equilibrium constant for the reaction shown in the equation:
2NOBr(g) (equilibrium Arrow) 2NO(g) + Br2 (g)
kk,
n(NOBr)in equilibrium= cxv=0.075x5=0.375
n(NO)produced=n(NOBr)consumed=n(NOBr)initial-n(NOBr)in equilibrium=2-0.375=1.625
n(Brs)produced=1/2n(NO)produced=0.8125
c(NOBr)=0.075, c(NO)=1.625/5=0.325,C(Br2)=0.8125/5=0.1625
0.325^2 x 0.1625 / 0.075^2 gives 3.05 =]
Post by: vamsiaus on July 18, 2009, 02:39:57 pm
Post by: vamsiaus on July 18, 2009, 02:57:08 pm
Water undergoes self ionistion according to the following equation.
2H20 (l) (eq. arrow) H30+ (l) + OH- (aq) delta h > 0
The pH of pure wter at 10 degress is
A. less than 7
B. greater than 7
C. Equal to 7
D. Greater thanor less than 7 depending upon the source of the water
If someone could explain why one answer is the right one, it would be greatly appreciated.
Thanks.
Post by: TrueTears on July 18, 2009, 03:09:19 pm
As the temp decreases the back reaction is preferred. [As it releases heat]
Now that means less products are formed. Less
Post by: vamsiaus on July 18, 2009, 03:14:04 pm