# 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?