The rate law for the reaction 2MnO4 +5HSO3+H2Mn²+ +55042+ 3H₂O is Rate - k[MnO4][HSO3 ]²[H]. One experiment, run at 20°C, measured the rate of reaction to be 7.2x10-6 mol L¹s¹ when the reactant concentrations were [MnO4]-0.020M, [HSO3]-3.0x10 ³M and [H*] -0.010M. The value of the rate constant for this reaction can be calculated to be (units left out on purpose) O 6.0x10² O 2.5x 104 O 12 O 4.0x 10³
The rate law for the reaction 2MnO4 +5HSO3+H2Mn²+ +55042+ 3H₂O is Rate - k[MnO4][HSO3 ]²[H]. One experiment, run at 20°C, measured the rate of reaction to be 7.2x10-6 mol L¹s¹ when the reactant concentrations were [MnO4]-0.020M, [HSO3]-3.0x10 ³M and [H*] -0.010M. The value of the rate constant for this reaction can be calculated to be (units left out on purpose) O 6.0x10² O 2.5x 104 O 12 O 4.0x 10³
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![The rate law for the reaction 2MnO4 +5HSO3+H2Mn²+ +55042+ 3H₂O is Rate - k[MnO4][HSO3 ]²[H]. One experiment, run at
20°C, measured the rate of reaction to be 7.2x10-6 mol L¹s¹ when the reactant concentrations were [MnO4]-0.020M,
[HSO3]-3.0x10 ³M and [H*] -0.010M. The value of the rate constant for this reaction can be calculated to be (units left out on
purpose)
O 6.0x10²
O 2.5x 104
O 12
O 4.0x 10³](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F885ad811-e1fc-4fdd-9f4a-b82767372835%2F44348928-55c0-43ce-8eec-4e50973cdb09%2Fpw40sod_processed.png&w=3840&q=75)
Transcribed Image Text:The rate law for the reaction 2MnO4 +5HSO3+H2Mn²+ +55042+ 3H₂O is Rate - k[MnO4][HSO3 ]²[H]. One experiment, run at
20°C, measured the rate of reaction to be 7.2x10-6 mol L¹s¹ when the reactant concentrations were [MnO4]-0.020M,
[HSO3]-3.0x10 ³M and [H*] -0.010M. The value of the rate constant for this reaction can be calculated to be (units left out on
purpose)
O 6.0x10²
O 2.5x 104
O 12
O 4.0x 10³
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