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
Isn't the rate
-d(Cl2)/dt and -(1/3)d(F2)/dt?
If that is so, then
-d(Cl2)/dt = -(1/3)d(F2)/dt and that look like which one
To determine the equation that describes the relationship between the rates at which Cl2 and F2 are consumed in the given reaction, we need to analyze the coefficients of the balanced chemical equation.
The balanced chemical equation is:
Cl2(g) + 3F2(g) → 2ClF3(g)
The coefficients of Cl2 and F2 are 1 and 3, respectively. These coefficients represent the stoichiometric ratio between the reactants and products in the reaction.
Now, let's consider the rate of change of Cl2 and F2, represented by -d(Cl2)/dt and -d(F2)/dt, respectively. The negative sign indicates that the reactants are being consumed.
According to the stoichiometry of the reaction, 1 mole of Cl2 reacts with 3 moles of F2 to produce 2 moles of ClF3. Therefore, for every 1 mole of Cl2 consumed, we need 3 moles of F2 to be consumed.
Based on this information, we can conclude that the equation that describes the relationship between the rates at which Cl2 and F2 are consumed is:
3[-d(Cl2)/dt] = -d(F2)/dt
So, the correct answer is option c):
3[-d(Cl2)/dt] = -d(F2)/dt