Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?
Cl2(g) + 3F2(g) yield 2ClF3(g)
a)-d(Cl2)/dt = -d(F2)/dt
b)-d(Cl2)/dt = 2[-d(F2)/dt]
c)3[-d(Cl2)/dt] = -d(F2)/dt
d)2[-d(Cl2)/dt] = -d(F2)/dt
e)-d(Cl2)/dt = 3[-d(F2)/dt]
is it e
of those E looks like the best option but it should be:
-d(Cl2)/dt=-1/3[d(F2)/dt]
To find the equation that describes the relationship between the rates at which Cl2 and F2 are consumed in the given reaction, you need to use the balanced equation and the stoichiometry of the reaction.
The balanced equation is: Cl2(g) + 3F2(g) → 2ClF3(g)
The stoichiometry of the reaction tells us that for every one mole of Cl2 consumed, three moles of F2 are consumed, and two moles of ClF3 are produced.
Now let's consider the rates of consumption of Cl2 and F2, which can be represented as -d(Cl2)/dt and -d(F2)/dt, respectively. The negative sign represents the consumption or decrease in the concentration of Cl2 and F2 with respect to time (dt).
According to the stoichiometry, for every one mole of Cl2 consumed, three moles of F2 are consumed. Therefore, the equation that describes their relationship is:
- d(Cl2)/dt = 3(- d(F2)/dt)
This equation states that the rate of consumption of Cl2 is equal to three times the rate of consumption of F2.
So the correct answer is:
c) 3[-d(Cl2)/dt] = -d(F2)/dt