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
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?
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Rate Law concept. You can view video lessons to learn Rate Law. Or if you need more Rate Law practice, you can also practice Rate Law practice problems.