Heeded for this question. The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+ I2 → 2 HI Experiment [H₂0, M 0.0250 0.0250 0.0500 0.0500 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-1 [12]0, M Initial Rate, M-s¯¹ 0.0146 6.90 x 10-22 0.0292 1.38 x 10-21 0.0146 1.38 x 10-21 0.0292 2.76 x 10-21 S
Heeded for this question. The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+ I2 → 2 HI Experiment [H₂0, M 0.0250 0.0250 0.0500 0.0500 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for 1 2 3 4 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = M-1 [12]0, M Initial Rate, M-s¯¹ 0.0146 6.90 x 10-22 0.0292 1.38 x 10-21 0.0146 1.38 x 10-21 0.0292 2.76 x 10-21 S
Chemistry
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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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![The following initial rate data are for the gas phase reaction of hydrogen with iodine:
\[ \text{H}_2 + \text{I}_2 \rightarrow 2 \text{HI} \]
| Experiment | [H₂]₀, M | [I₂]₀, M | Initial Rate, M·s⁻¹ |
|------------|----------|----------|----------------------|
| 1 | 0.0250 | 0.0146 | 6.90 × 10⁻²² |
| 2 | 0.0250 | 0.0292 | 1.38 × 10⁻²¹ |
| 3 | 0.0500 | 0.0146 | 1.38 × 10⁻²¹ |
| 4 | 0.0500 | 0.0292 | 2.76 × 10⁻²¹ |
Complete the rate law for this reaction in the box below.
Use the form:
\[ k[A]^m[B]^n \]
where '1' is understood for \( m \) or \( n \) and concentrations taken to the zero power do not appear. Don't enter 1 for \( m \) or \( n \).
Rate = \_\_\_\_
\( k = \_\_ \)
M⁻¹·s⁻¹](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb8d8ce1c-d1ae-4fbf-bbe3-121c6915374e%2F337fd830-8dc4-47ea-baf9-9ecceff83e4e%2F9n1916d_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The following initial rate data are for the gas phase reaction of hydrogen with iodine:
\[ \text{H}_2 + \text{I}_2 \rightarrow 2 \text{HI} \]
| Experiment | [H₂]₀, M | [I₂]₀, M | Initial Rate, M·s⁻¹ |
|------------|----------|----------|----------------------|
| 1 | 0.0250 | 0.0146 | 6.90 × 10⁻²² |
| 2 | 0.0250 | 0.0292 | 1.38 × 10⁻²¹ |
| 3 | 0.0500 | 0.0146 | 1.38 × 10⁻²¹ |
| 4 | 0.0500 | 0.0292 | 2.76 × 10⁻²¹ |
Complete the rate law for this reaction in the box below.
Use the form:
\[ k[A]^m[B]^n \]
where '1' is understood for \( m \) or \( n \) and concentrations taken to the zero power do not appear. Don't enter 1 for \( m \) or \( n \).
Rate = \_\_\_\_
\( k = \_\_ \)
M⁻¹·s⁻¹
Expert Solution
Step 1
Rate law of an equation is determined by the rate constant and concentration of reactants .
In this case firstly we will determine the value of m, n and with the help of that we will determine rate law and rate constant.
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