Consider the reaction 2N₂O(g)$\rightarrow$2N₂(g)+ O₂(g) Rate = k[N₂O]For an initial concentration of N₂O of 0.50 M,What is the concentration of N₂O remaining after 2.0 min if k = 3.4 * 10^-³ s^-¹? A) 0.50 M B) 0.55 M C) 0.66 M D) 0.33 M E) 0.17 M

Question

Quizplus · Accepted Answer

Using first-order rate equation: ln([N₂O]/[N₂O]0) = -kt ln([N₂O]/0.50) = -(3.4*10^(-3)s^(-1))(2.0min)(60s/min) ln([N₂O]/0.50) = -0.40824 [N₂O]/0.50 = e^(-0.40824) [N₂O] = (0.50)e^(-0.40824) [N₂O] = 0.33 M (rounded to two significant figures)

Consider the Reaction 2N2O(g) →\rightarrow→ 2N2(g)+ O2(g) Rate = K[N2O]For an Initial Concentration of N2O

Consider the Reaction
2N₂O(g) $\rightarrow$ 2N₂(g)+ O₂(g)
Rate = K[N₂O]For an Initial Concentration of N₂O