SUUUPPEERR HARD. I have no idea how to do this one. Please include work for all
ID: 2242861 • Letter: S
Question
SUUUPPEERR HARD. I have no idea how to do this one. Please include work for all credit and points. WILL RATE!
A sealed bottle at 1 atm of pressure holds 1 mole of neon and 1 mole of argon gas at a temperature of 295 K. The curves show the distributions of velocities of the molecules of each gas. Find the molecules of neon which have velocities between 750 and 1000 (m/s). Find the volume of the bottle. In the bottle, vrms of the neon molecules is 603.9 m/s. The temperature is increased by 20.4o deg C, find the new vrms of these molecules. Find the new pressure in the bottle after this increase in temperature (in atm).
Explanation / Answer
A. A= 1/2 (b1+b2) h
A= 1/2 (b1+b2) (1000 m/s -750 m/s) I cannot see what the curve shows, but add the two numbers.
B. PV=nRT
P= 1 atm
n= # moles of neon + # of moles argon, which is 2
R= 0.0821
T= 295K to Celsius is 21.85 C.
21.85 C + 20.4 C = 42.25 C
42.25 C to Kelvin is 315.4 K
V= (2*0.0821*315.4K) / 1 atm = 51.78868m^3
C. Use vrms = (3RT/M)^(1/2)
R= constant 8.3145
M= molecular mass of Neon (20.1797)
(3*8.3145* 315.4K) / (20.1797 / 1000) ^(0.5)
== 6.244 x 10^2 m/s
D. PV=nRT
P * 51.79 = 2 * 0.082 * 315.4K
P= 0.998756 atm or 1.00 atm
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