BIOM 121 1nd Edition Lecture 10Outline of Last Lecture I. In-Class QuestionsOutline of Current Lecture I. In-class QuestionsII. Integrated Rate EquationsCurrent Lecture- Integrated Rate Equationo aA productso Rate = -1Δ[A]aΔto Ant that for a first order reaction: Rate = k[A] -1Δ[A] = k[A]a Δt -(ln[A]t – ln[A]0) = ak(t – 0) - Simplified: ln[A]0 – ln[A]t = akt- Ln[A]0 = akt [A]2- Zeroeth order: [A]0- [A]t = akt- Second order: 1 – 1 = akt[A]t [A]01. In the past, cyclopropane, C3H6, was used in a mixture with oxygen as an anesthetic. When heated, cyclopropane rearranges to propene in a first-order process. The rate constant for this reaction is 2.42/hr at 500° CIf the initial concentration of cyclopropane is 0.050 mol/L, how much time (in hours) must elapse for its concentration to drop to 0.010 mol/L?These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Answer: 0.67 hours2. The decomposition of ammonia on a metal surface to form nitrogen gas and hydrogen gas is a zero-order reaction. At 873° C, the value of the rate constant is 1.5x10-3 mol/Lsec. How long will it take to completely decompose 1.00 grams of ammonia in a 1.00 L flask?Answer: 2.0x101 seconds3. The rate constant for the decomposition of nitrogen dioxide at a high temperature is 3.40 L/molmin. Determine the time needed for the concentration of NO2 to decrease from 2.00 mol/L to 1.50 mol/LNO2(g) NO(g) + ½ O2(g)Answer: To be answered next
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