General Chemistry 2, Little Help needed!
I have 4 problems, which of i have done most of all but number 3. Just stuck here and there in all problems.
[ Concentrations (Mol/L) ] [ Mol / L * Sec ]
[CH3COCH3] [Br2] [H+] [Initial Rate]
0.30 0.05 0.05 5.7 X 10
-5 0.30 0.10 0.05 5.7 X 10
-5 0.30 0.05 0.10 12.0 X 10
-5 0.40 0.05 0.20 31.0 X 10
-5 0.40 0.05 0.05 7.6 X 10
-5 1) CH3COCH3 + Br2 + H+ :rarrow:CH3COCH2Br + Br-
a) Determine Rate expression, Give rate order with respect to each reactant as well as the overall rate order.
What i got -> Rate 3 / Rate 1, ( 12.0 X 10
-5Mol/L*Sec ) / ( 5.7 X 10
-5Mol/L*Sec )
= ( K (.30 )
x (.05)
y (.10)
z ) / ( K (.30)
x (.05)
y (.05)
z )
So, Rate 3/ Rate 1 = 2.1, (close to 2) and (.10 / .05)
z = 2
So, Z = 2 (Correct?)
-> Rate 5/ Rate 1, I get X = 1 (Correct?)
-> Rate 2/Rate 1, I get y = 2 (Correct?)
b) Determine Value for Rate Constant K with correct units.
What i got -> K = Rate / [CH3COCH3]
1[Br2]
2[H+]
1 (Once someone answers and i make sure part a is correct, ill know the part b values)
c) Determine Initial Rate of reaction When [H+] = .05 M [CH3COCH3] & [Br2] = .10 M
What i got -> Rate = ( K (from part b) ) (.50M)(.10M)
2(.10M)
(Once again, continuing from part b, just need to make sure part b is right)
2) The First order Rate Constant for the reaction A
B has been measured at a series of temperatures:
K ( s
-1 ) T (
oC )
10.6 10
47.4 20
162 30
577 40
-> Determine GRAPHICALLY the activation energy (Ea) for the reaction.
What i got -> I graphed the points and graph is curve going up. but i just dont know how/where to drive the problem to after that.
If little bone/hint/help tossed here will be appreciated.
Thank you in advance.