Consider this reaction: 8A(g) + 5B(g) $\rightarrow$8C(g) + 6D(g) If [C] is increasing at the rate of 4.0 mol L¯¹s¯¹, at what rate is [B] changing?

Question

Quizplus · Accepted Answer

According to the reaction stoichiometry, the coefficient ratio of B to C is 5:8. Therefore, if [C] is increasing at a rate of 4.0 mol L¯¹s¯¹, the rate of change of [B] can be calculated as follows: 
(rate of change of [B]) = (rate of change of [C]) × (coefficient ratio of B to C) ÷ 5 
= 4.0 × 8 ÷ 5 
= 6.4 mol L¯¹s¯¹ (negative since [B] is decreasing) 
Therefore, the best choice is B.

Consider This Reaction: 8A(g) + 5B(g) →\rightarrow→ 8C(g) + 6D(g) If [C] Is Increasing at the Rate

Consider This Reaction: 8A(g) + 5B(g) $\rightarrow$ 8C(g) + 6D(g) If [C] Is Increasing at the Rate