Which of the following equations correctly describes the relationship between the rate at which NO2 and Cl2 are consumed in the following reaction?
2 NO2(g) + Cl2(g) → 2 NO2Cl(g)
A. -d(NO2)/dt = 1/2 [d(Cl2)/dt]
B. -d(NO2)/dt = 2 [d(Cl2)/dt]
C. -d(NO2)/dt = 2 [-d(Cl2)/dt]
D. -d(NO2)/dt = 1/2 [-d(Cl2)/dt]
E. -d(NO2)/dt = -d(Cl2)/dt
-d(NO2)/dt = 2 [-d(Cl2)/dt]
thx answer is correct
To determine the relationship between the rate of consumption of NO2 and Cl2 in the given reaction, we need to consider the stoichiometry of the reaction.
Looking at the balanced equation:
2 NO2(g) + Cl2(g) → 2 NO2Cl(g)
We can see that the coefficients in the balanced equation represent the stoichiometric relationship between the reactants and products.
From the balanced equation, we can conclude that for every 2 moles of NO2 consumed, 1 mole of Cl2 is consumed.
Therefore, the correct relationship between the rate at which NO2 and Cl2 are consumed is:
-d(NO2)/dt = 1/2 [-d(Cl2)/dt]
So, the correct answer is option D.
To determine the relationship between the rate at which NO2 and Cl2 are consumed in the given reaction, we can examine the stoichiometry of the balanced equation.
The balanced equation represents the molar ratios of the reactants and products in the reaction. From the balanced equation:
2 NO2(g) + Cl2(g) → 2 NO2Cl(g)
We can see that it takes 2 moles of NO2 to react with 1 mole of Cl2, and this produces 2 moles of NO2Cl.
Based on the stoichiometry, the rate at which NO2 is consumed is twice the rate at which Cl2 is consumed. However, it's important to remember that rates are expressed as negative values since they represent the decrease in concentration over time.
Therefore, the correct equation that describes the relationship between the rate at which NO2 and Cl2 are consumed is:
-D(NO2)/dt = -2 * D(Cl2)/dt
Therefore, the correct answer is option E. -d(NO2)/dt = -d(Cl2)/dt.