This and the next question pertain to the following situation. A quantity of mol

Question

This and the next question pertain to the following situation.
A quantity of molecular hydrogen (H2) gas fills a one liter container at a temperature of 200 K and pressure of 1 atm.

What is the average (rms) speed of the molecules?

(a) 16 m/s
(b) 74 m/s
(c) 274 m/s
(d) 1600 m/s
(e) 4570 m/s




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QUESTION 6*
How much internal energy is in the hydrogen?
(a) 1 l-atm
(b) 1.5 l-atm
(c) 2.5 l-atm
(d) 3.0 l-atm
(e) 3.5 l-atm





QUESTION 15**
Let two different (and not necessarily ideal) gases (X and Y) at fixed equal temperature be confined to opposite sides of a fixed-volume cylinder with a sliding piston in between. In thermal equilibrium, which one of these equations holds (with the usual definitions of the symbols)?
(a) sA = sB
(b) dOA / dVA = dOB / dVB
(c) dsA / dVA = dsB / dVB

Explanation / Answer

you only need the temp for this one...

   v rms = sqrt (3 R T / M) = sqrt (3*8.314*200 / 0.002) =

                 = 1579 m/s = 1600 m/s

6) total energy = (5/2) nRT = (5/2) pV = (5/2) * 1 * 1 =

            = 2.50 atm-L

15) This one is sneaky... they tell you that the pressures and temperatures of both gases are the same. This means that, using pV = nRT, the ratio of   n/V is the same for both gases.

The rate of change of entropy with volume is defined as   ds/dV = nR/V  

So this must be the same for both sides...   (ds/dV)A = (ds/dV)B... the answer is (c)

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