An ideal gas is heated under constant pressure (Pext = 2 bar) from an initial volume of 1 liter and temperature 250C to a final temperature of 370C. what is the final volume of the gas? how many moles of gas are involved?
Please note the temperatures (temperature 250C to a final temperature of 370C considered) mentioned.
=====An ideal gas is heated under constant pressure (Pext = 2 bar) from an initial volume of 1 liter and temperature 250C to a final temperature of 370C. what is the final volume of the gas? how many moles of gas are involved?====
At constant pressure, from the gas laws we know,
P1V1/T1 = P1V2/T2,
or V1T2 = V2T1
Where 1 stands for initial and 2 for final,
V1 = 1 L
T1 = 250C = 298 K and T2 = 370C = 310 K
V2 =?
From the above formula, V2= 1*310/298 L = 1.0403 L is the final volume.
Again, from the gas laws, we can write,
PV=nRT
By replacing the initial state values and considering R= 0.082 L atm / mol K
we get, n = 1.97385*1/0.082/298 ( 2 bar = 1.97385 atm) = 0.0808 moles of gas was present.
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