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Calculate the number of gas molecules in a container of volume 0.25 m3 filled with gas under a partial vacuum of pressure 10 Pa at 22 degree C. If 6.10 moles of a monatomic ideal gas at a temperature of 280 K arc expanded isothermally from a volume of 1.33 L to a volume of 3.75 L, calculate the heat flow into or out of the gas J Suppose 173 moles of a monatomic ideal gas undergoes an isothermal expansion as shown in the figure. (The horizontal axis is marked in increments of 20 m3.) How much work is done by the gas during this expansion? J Eleven moles of an ideal monatomic gas expand isothermally at a temperature of 15 degree C. If the volume of the gas quadruples during this process, what is the heat flow into the gas? kJ Three moles of a monatomic ideal gas are heated at a constant volume of 2.50 m3. The amount of heat added is 4.86 times 103 J. Determine the change in pressure.

Explanation / Answer

6. First find the number of moles, n:

PV = nRT ==> n = PV / RT

22 C + 273 C = 295 K

n = (10 Pa / 101325 Pa) (0.25 m^3)(1000) / (0.082 L-atm/ mol K) (295 K)

n = (9.87 x 10^-5) (250) / 24)

n = 1.028 x 10^-3 mol

Now, get molecules of gas: (1.028 x 10^-3 mol) ( 6.022 x 10^23) = 6.19 x 10^20 molecules of gas [ANS]

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7. This one is pretty easy if you know this equation:

W = nRT ln (V2/ V1)

W = (6.10 mol) (8.3144 J/mol.K) (280 K) ln (3.75 L / 1.33 L)

W = Q (since this is an isothermal process)

Q = 1.47 x 10^4 J [ANS]

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8. Again, the equation for Work is handy, and we can find final and initial volume from the graph (V2 and V1, respectively). However, we need to find the temperature. The cool thing is, during isothermal process, temperature is constant, so T1 and T2 (initial and final temperature doesn

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