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Chapter 5: Q 5.74 (page 202)
Check that equations 5.69 and 5.70 satisfy the identity (equation 5.37)
Hence, the identity is satisfied.
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Let the system be one mole of argon gas at room temperature and atmospheric pressure. Compute the total energy (kinetic only, neglecting atomic rest energies), entropy, enthalpy, Helmholtz free energy, and Gibbs free energy. Express all answers in SI units.
Write down the equilibrium condition for each of the following reactions:
Derive the van't Hoff equation,
which gives the dependence of the equilibrium constant on temperature." Here is the enthalpy change of the reaction, for pure substances in their standard states (1 bar pressure for gases). Notice that if is positive (loosely speaking, if the reaction requires the absorption of heat), then higher temperature makes the reaction tend more to the right, as you might expect. Often you can neglect the temperature dependence of; solve the equation in this case to obtain
As you can see from Figure5.20,5.20,the critical point is the unique point on the original van der Walls isotherms (before the Maxwell construction) where both the first and second derivatives ofPPwith respect toVV(at fixedTT) are zero. Use this fact to show that
When solid quartz "dissolves" in water, it combines with water molecules in the reaction
(a) Use this data in the back of this book to compute the amount of silica dissolved in water in equilibrium with solid quartz, at 25掳 C
(b) Use the van't Hoff equation (Problem 5.85) to compute the amount of silica dissolved in water in equilibrium with solid quartz at 100掳C.
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