6. Consider the overall reaction: 2 NO (g) + Cl₂ (g) 2 NOCI (g) given the following initial rates of reaction measured for the given concentrations of species: [NO] (M) [Cl₂] (M) 0.50 Experiment Number Rate (M/hr) 1.00 1.00 2 3 1.19 2.39 9.58 a) Determine the reaction order for each reactant. (Observe first!) (Don't use the coefficients for granted. Show steps.) NO₂- Scond Cl2- first NOCI - second need. Calculation. 0.50 0.50 1.00 reaction orders don't come from equation. b) Write the rate law for THIS reaction. (NOT general rate law with x and y. Use the reaction orders you determined. TACAD 16 ACB AL ACO SO a ot 2 Ot c) Calculate the rate constant for this reaction. (Note the unit.) d) Calculate the rate when [NO] and [Cl₂] are both 2.50 M. At

Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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6. Consider the overall reaction: 2 NO (g) + Cl₂ (g) 2 NOCI (g)
given the following initial rates of reaction measured for the given concentrations of species:
Experiment Number Rate (M/hr)
[Cl₂] (M)
[NO] (M)
0.50
1.00
1.00
1
1.19
2.39
9,58
a) Determine the reaction order for each reactant. (Observe first!) (Don't use the coefficients for granted. Show steps.)
NO₂- Scond
Cl2 - first
NOCI - second.
need. Calculation.
0.50
0.50
1.00
b) Write the rate law for THIS reaction. (NOT general rate law with x and y. Use the reaction orders you determined.)
1 ACAD
reaction orders don't come from equation.
ACB
16
AD
ACO SO
a ot
- 2
H
Ot
c) Calculate the rate constant for this reaction. (Note the unit.)
d) Calculate the rate when [NO] and [Cl₂] are both 2.50 M.
Transcribed Image Text:6. Consider the overall reaction: 2 NO (g) + Cl₂ (g) 2 NOCI (g) given the following initial rates of reaction measured for the given concentrations of species: Experiment Number Rate (M/hr) [Cl₂] (M) [NO] (M) 0.50 1.00 1.00 1 1.19 2.39 9,58 a) Determine the reaction order for each reactant. (Observe first!) (Don't use the coefficients for granted. Show steps.) NO₂- Scond Cl2 - first NOCI - second. need. Calculation. 0.50 0.50 1.00 b) Write the rate law for THIS reaction. (NOT general rate law with x and y. Use the reaction orders you determined.) 1 ACAD reaction orders don't come from equation. ACB 16 AD ACO SO a ot - 2 H Ot c) Calculate the rate constant for this reaction. (Note the unit.) d) Calculate the rate when [NO] and [Cl₂] are both 2.50 M.
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