Use the van der Waals equation and the ideal gas equation to
calculate the volume of 1.000 mol of neon at a pressure of 500.0
bar and a temperature of 355.0 K. (Hint: One way to solve the van
der Waals equation for V is to use successive approximations. Use
the ideal gas law to get a preliminary estimate for V
V in ideal gas
V in van der waal gas
Van der Waals Gases
Under what conditions of volume does a van der Waals gas behave
like an ideal gas? Use the van der Waals equation of state to
justify your answer.
In the van der Waals model of a gas, as compared to an ideal
gas,
a. Intermolecular forces decrease the pressure, but
finite molecular volume increases it
b. Both intermolecular forces and finite molecular
volume increase the pressure
c. Both intermolecular forces and finite molecular
volume decrease the pressure
d. Intermolecular forces increase the pressure, but
finite molecular volume decreases it
Explain your answer.
Internal Energy (U); Enthalpy (H); Helmholtz Free Energy (A or
F); Gibbs Free Energy (G),
which one is most appropriate for a problem on
a) Explosions
b) Skin Permeation of Chemicals
c) Rubber Elasticity
d) Distillation Columns
The van der Waals equation for 1 mole of gas is given by (p
+av-2)(v - b) = RT. In general, curves of p versus v
forvarious values of T exhibit a maximum and a minimum at the
twopoints where (δp/δv)T = 0. The maximum and minumum
coalesceinto a single point on that curve
where(δ2p/δv2)T = 0 inaddition to
(δp/δv)T = 0. This point is calledthe "critical point"
of the substance and its temperature,pressure, and molar volume are
denoted by...
1. Calculate the standard reaction entropy, enthalpy and Gibbs
free energy for the following reactions
a) N2(g) + NO2(g) ---> NO(g) + N2O(g) and
b) 2F2(g) +2H2O(l) ---> 4HF(aq) + O2(g)
what is the change in entropy, enthalpy and gibbs free energy
when 1 L of ideal gas i, 3 L of ideal gas j and 4 L of ideal gas k,
each at 1 atm and room temperature (298.15K) blend to form a gas
mixture at the same conditions?