Problem: The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 3.48× 10–10 cm3·molecule–1·s –1 at 298 K.1. Convert the rate constant to units of M –1·s –1.2. Convert the rate constant to units of Torr–1·s –1.3. What is the order of this reaction?

FREE Expert Solution

Part 1) We're being asked to convert the rate constant to units of M –1·s –1.

Given: k = 3.48×10–10 cm3·molecule–1·s –1 = 3.48×10–10 cm3/(molecule·s)

Recall that M = mol/L → M-1 = L/mol

Conversion factors needed: 

1 mol = 6.022×1023 molecules
1 cm = 10–1 dm
1 dm3 = 1 L

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Problem Details

The National Institute of Science and Technology (NIST) kinetics database lists the rate constant, k, of a particular gaseous reaction as 3.48× 10–10 cm3·molecule–1·s –1 at 298 K.

1. Convert the rate constant to units of M –1·s –1.

2. Convert the rate constant to units of Torr–1·s –1.

3. What is the order of this reaction?

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