For a #"313 g"# sample of helium gas that cools by #41.6^@ "C"# due to being compressed by #"267 L"# at a constant external pressure of #"1 atm"#, if its molar heat capacity is #"20.8 J/mol"^@ "C"#, calculate #DeltaE#, #q#, #w#, and #DeltaH#?
1 Answer
Yep, this is going to be long. So bear with me! Knowing your derivations would really help here...
Well, first of all, let's get the pressure in terms of
#P = "1.01325 bar"#
Alright, so... evidently we should know the first law of thermodynamics if we have to solve for all three of these:
#\mathbf(DeltaE = q + w)# where
#DeltaE# is the change in internal energy caused by heat flow#q# and work#w = -P int_(V_1)^(V_2) dV# .
The next thing we should know is how work is defined. We know that the temperature decreased, and that it doesn't matter what
We know that the gas was compressed, so from the perspective of the gas, work was done on the gas. That means the gas let something else work upon it. Thus, the work will turn out to be numerically positive (a negative
Also, I guess since the pressure is constant, using a convenient thermodynamics relation:
#DeltaH = DeltaE + Delta(PV)#
#= q + w + (PDeltaV + VDeltaP + DeltaPDeltaV)#
#= q - cancel(PDeltaV) + cancel(PDeltaV) + cancel(VDeltaP + DeltaPDeltaV)^(DeltaP = 0)#
#\mathbf(DeltaH = q_p)# in
#"J"# .
Now what about that molar heat capacity
#((delbarH)/(delT))_P = barC_P#
(the partial derivative of the molar enthalpy with respect to the temperature at a constant pressure is the molar heat capacity.)
Thus, at a constant pressure:
#dbarH = barC_PdT#
#\mathbf(DeltabarH = int_(T_1)^(T_2) barC_P dT)# in
#"J/mol"# (not#"J"# ).
Since the heat capacity will stay pretty much linear in this temperature range (we have to assume that just because we aren't given the equation... though you can probably look it up in the NIST database):
#n_"He"DeltabarH = color(blue)(q_p = n_"He"barC_PDeltaT)#
where
Note that
#\mathbf(barC_P ne C_P)#
Now we need
#w = -P int_(V_1)^(V_2) dV#
#color(blue)(w = -P(V_2 - V_1))# in
#"L"cdot"bar"# , which you can convert to#"J"# (Wikipedia the universal gas constant#R# in#("L"cdot"bar")/("mol"cdot"K")# and compare it in#"J"/("mol"cdot"K")# ).
And finally:
#color(blue)(DeltaE) = q_p + w#
#= color(blue)(n_"He"barC_PDeltaT - P(V_2 - V_1))# where
#V_2 < V_1# . You can probably tell by now that the units are, of course,#"J"# .
Yep, that's all of it! Just use these numbers you've been given, and that should be it.
#barC_P = "20.8 J/mol"^@ "C"#
#P = "1.01325 bar"#
#DeltaT = -41.6^@ "C"#
#DeltaV = -"267 L"#
#n_"He" = "313" cancel"g He" xx "1 mol He"/("4.0026" cancel"g He") = ...#