Answer:
w= - 1.7173 kJ, q= 1.7173 kJ, q(rev) = 1717.3 J = 1.7173 kJ.
Explanation:
Okay, from the question we are given the information below;
Number of moles, n= 1 mole; initial volume, v(1) = 1.0 litres (L); pressure (p) = 5atm, final volume(v2) = 2.0 Litres(L) ; the workdone, w= not given; the heat, q and q(rev)= not given and the gas was said to expand isothermally.
So, this question is a question from the part of chemistry known as thermodynamics. Therefore, grip yourself we are delving into thermodynamics 'waters' now.
For expansion isothermally; the workdone, w= -nRT ln v2/v1.
Where T= temperature= 25° C = 298 k and R= gas constant.
Therefore; workdone, w = - 1 × 8.314 × 298 × ln(2/1).
Workdone,w= - 1717.32204643. =
- 1717.3 Joules (J).
==> Workdone,w= - 1.7173 kJ.
Then, we are to find q. q can be solved by using the first law of thermodynamics, which by mathematical representation is:
∆U= q + w. Where ∆U= change in internal enegy. Since the question is dealing with isothermal expansion, there is this rule that says for an isothermal expansion ∆U = 0.
Hence, 0 =q + [- 1717.3 Joules (J)].
q=1717.3 J = 1.7173 kJ.
Finally, the q(rev) which is= nRT ln (v2/V1).
q(rev) = 1 × 8.314 × 298 ln (2/1).
q(rev) = 1717.3 J = 1.7173 kJ.
PS: please note the negative signs in the workdone and the positive sign in the q(rev).
