Consider this reaction:
2NH₃(g) $\rightarrow$ N₂(g) + 3H₂(g) If the rate $\Delta$ [H₂]/ $\Delta$ t is 0.030 mol L¯¹ s¯¹, then $\Delta$ [NH₃]/ $\Delta$ t is:

Question

Consider this reaction: 2NH₃(g) $\rightarrow$N₂(g) + 3H₂(g) If the rate $\Delta$[H₂]/$\Delta$t is 0.030 mol L¯¹ s¯¹, then $\Delta$[NH₃]/$\Delta$t is:

Quizplus · Accepted Answer

The rate law for this reaction indicates that the rate of formation of N₂ and H₂ depends on the concentration of F1F1F1S1 in the reaction mixture. Since the rate of the reaction is provided for F1F1F1S1, we can use this information to calculate the rate of formation of N₂ and H₂. According to the balanced chemical equation, the stoichiometric ratio of F1F1F1S1 and NH₃ is 2:1. Therefore, the rate of formation of N₂ can be calculated by dividing the given rate by 2. This gives us (-0.030 mol L¯¹ s¯¹)/2 = -0.015 mol L¯¹ s¯¹. Similarly, the rate of formation of H₂ can be calculated by multiplying the rate of formation of N₂ by 3 (stoichiometric coefficient in the balanced equation). This gives us (-0.015 mol L¯¹ s¯¹) x 3 = -0.045 mol L¯¹ s¯¹. Therefore, the rate of the reaction with respect to NH₃ is -0.045 mol L¯¹ s¯¹. The correct choice is C.

Consider This Reaction: 2NH3(g) →\rightarrow→ N2(g) + 3H2(g) If the Rate

Consider This Reaction:
2NH₃(g) $\rightarrow$ N₂(g) + 3H₂(g) If the Rate