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?
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
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.
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.
-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
To determine the relationship between the rates at which Cl2 and F2 are consumed in the given reaction, we need to look at the stoichiometry of the balanced equation.
From the balanced equation:
(Cl)2 + 3(F)2 <=> 2(ClF)3
We can see that the coefficient of Cl2 is 1, and the coefficient of F2 is 3. This means that for every 1 mole of Cl2 consumed, 3 moles of F2 are consumed.
Now, let's define the rate of reaction for Cl2 as -d(Cl2)/dt (the negative sign indicates consumption), and the rate of reaction for F2 as -d(F2)/dt.
Since 1 mole of Cl2 is consumed for every 3 moles of F2 consumed, we can express the relationship between their rates based on their coefficients:
- d(Cl2)/dt = 1/3 * (-d(F2)/dt)
Therefore, the correct equation to describe the relationship between the rates at which Cl2 and F2 are consumed in the reaction is:
- d(Cl2)/dt = 1/3 * (-d(F2)/dt)