If the volume of an ideal gas is 22.5 L when it is at a temperature of 365 K, what will the volume be when the gas cools to 338K
1 answer:
Answer:
20.8L = Final volume of the gas
Explanation:
Based on Charles's law, the volume of a gas is directly proportional to the temperature of the gas under pressure constant. The equation is:
<em>where V is volume and T absolute temperature of 1, initial state and 2, final state.</em>
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If initial volume is 22.5L, initial T = 365K and final temperature 338K:
22.5L / 365K = V₂ / 338K
<h3>20.8L = Final volume of the gas</h3>You might be interested in
Answer:
(a)
(b)
(c)
Explanation:
Hello,
(a) In this case, since entropy remains unchanged, the constant should be computed for air as an ideal gas by:
Next, we compute the final temperature:
Thus, the work is computed by:
(b) In this case, since is given, we compute the final temperature as well:
And the isentropic work:
(c) Finally, for isothermal, final temperature is not required as it could be computed as:
Regards.
This problem is describing a gas mixture whose mole fraction of hexane in nitrogen is 0.58 and which is being fed to a condenser at 75 °C and 3.0 atm, obtaining a product at 3.0 atm and 20 °C, so that the removed heat from the system is required.
In this case, it is recommended to write the enthalpy for each substance as follows:
Whereas the specific heat of liquid and gaseous n-hexane are about 200 J/(mol*K) and 160 J/(mol*K) respectively, its condensation enthalpy is 31.5 kJ/mol, boiling point is 69 °C and the specific heat of gaseous nitrogen is about 29.1 J/(mol*K) according to the NIST data tables and and
are the mole fractions in the gaseous mixture. Next, we proceed to the calculation of both heat terms as shown below:
It is seen that the heat released by the nitrogen is neglectable in comparison to n-hexanes, however, a rigorous calculation is being presented. Then, we add the previously calculated enthalpies to compute the amount of heat that is removed by the condenser:
Finally we convert this result to kJ:
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