chemistry

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?

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  1. 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.

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  2. 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.

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  3. -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

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  4. 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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    posted by kris

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