Q2 Sulfur dioxide is oxidised by oxygen to form sulfur trioxide. This reaction is described by the following equation: 2 SO₂ + 0₂ The reaction was studied at 55°C and the data in the table were collected. [SO₂] 1.53 0.17 0.51 1.53 x= 2 SO3 y= [0₂] 0.42 0.21 0.42 0.84 The rate law for the reaction can be written as: rate = k[SO₂]*.[0₂] Determine the orders x and y and calculate the rate constant k. Enter these values in the boxes below and select the correct units for the rate constant. Initial rate of reaction (M sec¹) 0.0527 0.00293 0.0176 0.105 sec O secl mol-² L² sec-1 mol-³ L³ sec-1 mol-¹ L sec-1
Q2 Sulfur dioxide is oxidised by oxygen to form sulfur trioxide. This reaction is described by the following equation: 2 SO₂ + 0₂ The reaction was studied at 55°C and the data in the table were collected. [SO₂] 1.53 0.17 0.51 1.53 x= 2 SO3 y= [0₂] 0.42 0.21 0.42 0.84 The rate law for the reaction can be written as: rate = k[SO₂]*.[0₂] Determine the orders x and y and calculate the rate constant k. Enter these values in the boxes below and select the correct units for the rate constant. Initial rate of reaction (M sec¹) 0.0527 0.00293 0.0176 0.105 sec O secl mol-² L² sec-1 mol-³ L³ sec-1 mol-¹ L sec-1
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.28PAE
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Sulfur dioxide is oxidised by oxygen to form sulfur trioxide. This reaction is described by the following equation:
2 SO₂ + O₂
The reaction was studied at 55°C and the data in the table were collected.
[SO₂]
1.53
0.17
0.51
1.53
x=
2 SO3
The rate law for the reaction can be written as: rate = k[SO₂]*. [0₂]
Determine the orders x and y and calculate the rate constant k. Enter these values in the boxes below and select the correct units for the rate constant.
k=
[0₂] Initial rate of reaction (M sec¹)
0.42
0.0527
0.21
0.00293
0.42
0.0176
0.84
0.105
sec
O sec-1
mol-² L² sec-1
mol-³ L³ sec-1
mol-¹ L sec-¹](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F32e6b975-0532-4261-be6c-6e0d4180a1ca%2F95178a8e-b3ec-4498-80d2-07f08bc19b38%2F2495g4w_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Q2
Sulfur dioxide is oxidised by oxygen to form sulfur trioxide. This reaction is described by the following equation:
2 SO₂ + O₂
The reaction was studied at 55°C and the data in the table were collected.
[SO₂]
1.53
0.17
0.51
1.53
x=
2 SO3
The rate law for the reaction can be written as: rate = k[SO₂]*. [0₂]
Determine the orders x and y and calculate the rate constant k. Enter these values in the boxes below and select the correct units for the rate constant.
k=
[0₂] Initial rate of reaction (M sec¹)
0.42
0.0527
0.21
0.00293
0.42
0.0176
0.84
0.105
sec
O sec-1
mol-² L² sec-1
mol-³ L³ sec-1
mol-¹ L sec-¹
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