Consider the following gas samples:
Sample A: S 2(g); n = 1 mol; T = 800 K; P = 0.20 atm; and
Sample B: O 2(g); n = 2 mol; T = 400 K; P = 0.40 atm
Which one of the following statements is FALSE?
a) The volume of sample A is twice the volume of sample B.
b) The average kinetic energy of the molecules in sample A is twice the average kinetic energy of the molecules in sample B.
c) The fraction of molecules in sample A having a kinetic energy greater than some high fixed value is larger than the fraction of molecules in sample B having kinetic energies greater than that same high fixed value.
d) The mean square velocity of molecules in sample A will be twice as large as the mean square velocity of molecules in sample B.
e) Assuming identical intermolecular forces in the two samples. sample A should be more nearly ideal than sample B.
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 Kinetic Energy of Gases concept. You can view video lessons to learn Kinetic Energy of Gases. Or if you need more Kinetic Energy of Gases practice, you can also practice Kinetic Energy of Gases practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofConsider the following gas samples:Sample A: S 2(g); n = 1 m...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Jules took 9 minutes and 12 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Perrin's class at UCSD.