### Reaction Rate Calculation for \(\text{Cl}_2 (g) + 3 \text{F}_2 (g) \rightarrow 2 \text{ClF}_3 (g)\)**Reaction Information:**- Given rate of change for \([\text{Cl}_2]\) is \(\Delta[\text{Cl}_2]/\Delta t = -0.054 \, M/s\).**Step-by-Step Calculation:**1. **Rate Equation:** \[ \text{rate} = -\frac{\Delta [\text{Cl}_2]}{\Delta t} = -\frac{1}{3} \frac{\Delta [\text{F}_2]}{\Delta t} = \frac{1}{2} \frac{\Delta [\text{ClF}_3]}{\Delta t} \]2. **Rearrange to Solve for \(\Delta[\text{ClF}_3]/\Delta t\):** \[ \frac{\Delta [\text{ClF}_3]}{\Delta t} = -2 \frac{\Delta [\text{Cl}_2]}{\Delta t} \] Substituting the given value: \[ = -2(-0.054 \, M/s) \] \[ = 0.11 \, M/s \]**Instructions:**- Determine the rate of the reaction.- Express your answer to two significant figures.- Include the appropriate units.**Input Box:**- Rate = [Value] [Units]**Hint:** Click "View Available Hint(s)" for additional guidance.

Given that: Cl2(g) + 3F2(g) ....> 2ClF3(g) d[Cl2]/dt = -0.054 M/s Here negative sign shows that , concentration of reactant decreases as time increases. Differential rate law for reaction: Rate = -d[Cl2]/dt = -1/3 d[F2]/dt = +1/2 d[ClF3]/dt So, Rate = -d[Cl2]/dt = 0.054 M/s Rate = 0.054 M/s

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MISSED THIS? Réad Séctión 15.2 (Page) ; Watch KCV 15.2, IWE 15.1. rate = - At 2 At Consider the reaction Then rearrange this equation to solve for A[CIF3]l/At: Cl2 (g) + 3F2 (g) → 2CIF3 (g), A[CI]/At = -0.054 M/s. A[CIF;] -2 At At -2(-0.054 M/s) 0.11 M/s Part C Determine the rate of the reaction. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) ? Value Units rate =

MISSED THIS? Réad Séctión 15.2 (Page) ; Watch KCV 15.2, IWE 15.1. rate = - At 2 At Consider the reaction Then rearrange this equation to solve for A[CIF3]l/At: Cl2 (g) + 3F2 (g) → 2CIF3 (g), A[CI]/At = -0.054 M/s. A[CIF;] -2 At At -2(-0.054 M/s) 0.11 M/s Part C Determine the rate of the reaction. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) ? Value Units rate =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Correct answers are given in second picture!!! Please show me how to get them and explain!
For the reaction: BrO3-(aq) + 5Br (aq) + 8H*(aq) → 3Br2(/) + H201) The initial rate of the reaction has been measured at the reactant concentration show: Trial [BrO;] (mol/L) 1 [H'] [Br ] Initial rat (mol/L) (mol/L) (mol/L-s) 0.10 0.10 0.10 8.0 0.20 0.10 0.10 16 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 The value for k will be: A L/mol.s Ouestion 13 (1 23
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For the hypothetical reaction A + 2B 3C, the rate of appearance of C given by (A[C]/At) may also be expressed as O A[C]/At = -(2/3) A[B]/At O A[C]/At = -(3/2) A[B]/At O A[C]/At = -(1/2) A[A]/At %3D O A[C]/At = A[A]/At
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O KINETICS AND EQUILIBRIUM Using a second-order integrated rate law to find concentration... -1-1 At a certain temperature the rate of this reaction is second order in Cl,0, with a rate constant of 103.Ms: 2Cl,0; (g) 2Cl, (g) +50, (g) → Suppose a vessel contains Cl,0, at a concentration of 0.130M. Calculate the concentration of Cl,0, in the vessel 0.550 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10 Check Explanation Terms of Use | Privacy Center Accessibility 2021 McGraw Hill LLC. All Rights Reserved. II