A high vacuum pump can produce a pressure of 1.0 × 10-6 Torr. How many molecules are in each mL of gas at 25 °?
A high vacuum pump can produce a pressure of 1.0 × 10-6 Torr. How many molecules are in each
mL of gas at 25 °C at this low pressure?
I know that this is an ideal gas problem but I'm stuck on figuring out n. If PV = nRT then n = PV/RT obviously, but how do I figure out where mL fit in? I tried converting torr to atm and an arbitrary number of 1000 mL for the volume and I get a number that's just absurd.
The correct answer is 3.2 x 10^10, but I need to know why.
Muchos gracias.
More Questions From This User See All
Answers & Comments
Verified answer
i used 1 mol for n (since we know there are 6.022e23 molecules per mole) and solved for V:
1e-6 torr (V) = 1 mol (62.36 L torr/mol K) (298 K)
V = 1.86e10 L
since 1 mol = 6.022e23 molecules:
6.022e23 molecules/1.86e10 L * L/1000 mL = 3.2e10 molecules/mL
Natural Penis Enlargement Guide - http://longpenis.uzaev.com/?IIvq