Asked by uci student

Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?

(Cl)sub2 + 3[(F)sub2] <=> 2 [ClFsub3]


i put -d(Cl2)/dt = 3[-d(F2)/dt] but apparently that isnt right, and im not quite sure why it isnt. could anyone push me in the appropriate direction?
Answered by DrBob222
If aA + bB ==> cC + dD,
rate of rxn = -(1/a)(dA/dt) = -1/b(dB/dt) etc.
So wouldn't rate of reaction equal
-(1)(dCl2/dt) = -(1/3)(dF2/dt) = (1/2)(dClF3/dt)
Check me out.
Answered by uci student
well yea, but the only responses listed are as follows:

-d(Cl2)/dt = 2[-d(F2)/dt]

-d(Cl2)/dt = 3[-d(F2)/dt]

2[-d(Cl2)/dt] = -d(F2)/dt

3[-d(Cl2)/dt] = -d(F2)/dt

-d(Cl2)/dt = -d(F2)/dt

and none of those make sense.
Answered by uci student
-d(Cl2)/dt = 3[-d(F2)/dt]

2[-d(Cl2)/dt] = -d(F2)/dt

3[-d(Cl2)/dt] = -d(F2)/dt

-d(Cl2)/dt = -d(F2)/dt
Answered by kris
3[-d(Cl2)/dt] = -d(F2)/dt

3 mol F2 are depleted for each 1 mol Cl2. Thus the rate of depletion of F2 is three times that of Cl2
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