At 55° the decomposition of N₂O₅ is first order,having a rate constant,k = 1.7 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 6.4 × 10^-3 M,the number of half-lives that are required for the N₂O₅ concentration to fall to 2.0 × 10^-⁴ M is ________,and the amount of time required is ________ minutes.

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The Answer of At 55° the decomposition of N₂O₅ is first order,having a rate constant,k = 1.7 × 10^-3 s^-1.If the initial concentration of N₂O₅ is 6.4 × 10^-3 M,the number of half-lives that are required for the N₂O₅ concentration to fall to 2.0 × 10^-⁴ M is ________,and the amount of time required is ________ minutes.

At 55° the Decomposition of N2O5 Is First Order,having a Rate

At 55° the Decomposition of N₂O₅ Is First Order,having a Rate