Use the experimental data to determine the rate law equation for the following reaction: Mg(s) + 12(g) → MgI2(s) Trial 1 2 3 Or=kMg||I₂|² Initial [Mg] (mmol/L) 0.06 0.06 0.12 Initial [12] (mmol/L) 0.23 0.46 0.23 Rate of Formation of MgCl2 (mmol/L-s) 3.40×10-3 1.36x10-2 6.80x10-3
Use the experimental data to determine the rate law equation for the following reaction: Mg(s) + 12(g) → MgI2(s) Trial 1 2 3 Or=kMg||I₂|² Initial [Mg] (mmol/L) 0.06 0.06 0.12 Initial [12] (mmol/L) 0.23 0.46 0.23 Rate of Formation of MgCl2 (mmol/L-s) 3.40×10-3 1.36x10-2 6.80x10-3
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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![Use the experimental data to determine the rate law equation for the following
reaction: Mg(s) + 12(g)
→ MgI2(s)
Trial
1
2
3
Or=k[Mg][1₂]²
Or=k [12] ²
Or=k[Mg] ² [1₂] ²
Or=k[Mg] [1₂]
Initial [Mg]
(mmol/L)
0.06
0.06
0.12
Initial [12]
(mmol/L)
0.23
0.46
0.23
Rate of Formation of
MgCl2 (mmol/L-s)
3.40×10-3
1.36x10-2
6.80x10-3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F373ad59d-f146-4bca-b118-d55d7a4ea0af%2Fa8b1c7d9-d646-41f3-8ee4-734e98f78fec%2Fkgwbygp_processed.png&w=3840&q=75)
Transcribed Image Text:Use the experimental data to determine the rate law equation for the following
reaction: Mg(s) + 12(g)
→ MgI2(s)
Trial
1
2
3
Or=k[Mg][1₂]²
Or=k [12] ²
Or=k[Mg] ² [1₂] ²
Or=k[Mg] [1₂]
Initial [Mg]
(mmol/L)
0.06
0.06
0.12
Initial [12]
(mmol/L)
0.23
0.46
0.23
Rate of Formation of
MgCl2 (mmol/L-s)
3.40×10-3
1.36x10-2
6.80x10-3
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