Which equation describes the relationship between the rates at which Cl2 and F2 are consumed in the following reaction?
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
You have not told us what the "following reaction" is. That makes all the difference.
To determine the relationship between the rates at which Cl2 and F2 are consumed in a reaction, we need to analyze the balanced chemical equation of the reaction. However, since the chemical equation is not provided, we cannot directly determine the correct answer option.
To clarify how to approach this type of problem in general, when we have a balanced chemical equation, we can compare the coefficients of the reactants to determine their relationship. The coefficients indicate the mole ratio between the reactants.
Let's say the balanced chemical equation for the reaction is:
aCl2 + bF2 → cX
In this equation, "a" and "b" represent the coefficients of Cl2 and F2, respectively. Since we are interested in the rates of consumption, we can represent their rates as:
-d(Cl2)/dt (the rate at which Cl2 is consumed)
-d(F2)/dt (the rate at which F2 is consumed)
Based on the balanced equation, we can compare the coefficients of Cl2 and F2 to determine their relationship.
In Option (e): -d(Cl2)/dt = 3[-d(F2)/dt], the coefficient of Cl2 is not related to the coefficient of F2.
Therefore, without knowing the balanced chemical equation, we cannot determine the correct answer option.