Consider the following reaction, 4𝑁𝐻3 + 3𝑂2 → 2𝑁2 + 6𝐻2𝑂 If the rate of formation of N2 is 2.00 𝑚𝑜𝑙 𝐿−1 𝑠−1, the rate at which NH3 reacts is:
A) 0.50 𝑚𝑜𝑙 𝐿−1 𝑠−1 B) 1.00 𝑚𝑜𝑙 𝐿−1 𝑠−1 C) 2.00 𝑚𝑜𝑙 𝐿−1 𝑠−1 D) 4.00 𝑚𝑜𝑙 𝐿−1 𝑠
Am I supposed to say its d since the mole ratio is 4:2
yes
To determine the rate at which NH3 reacts in the given reaction, we need to use the stoichiometry of the reaction. The balanced equation tells us that for every 4 moles of NH3 that react, 2 moles of N2 are formed.
From the given information, we know that the rate of formation of N2 is 2.00 mol L^-1 s^-1. Since the stoichiometry of the reaction is 4:2 for NH3:N2, the rate at which NH3 reacts is also 2.00 mol L^-1 s^-1.
Therefore, the correct answer is C) 2.00 mol L^-1 s^-1.