1 Million+ Step-by-step solutions

Calculate ∆tHo for the reaction NaCl (aq) + AgN03 (aq) → AgCI(s) + NaN03 (aq) from the information in Table 2.7 in the Data section.

Set up a thermodynamic cycle for determining the enthalpy of hydration of Ca2+ ions using the following data: enthalpy of sublimation of Ca (s), + 178.2 k] mol-1, first and second ionization enthalpies of Ca (g), 589.7 k] mol-1 and 1145 k] mol-1: enthalpy of vaporization of bromine, +30.91 kJ mol-1; dissociation enthalpy of Br2(g), + 192.9 k] mol-1; electron gain enthalpy of Br (g), -331.0 k] mol-1: enthalpy of solution of CaBr2(s), -103.1 k] mol-1: enthalpy of hydration of Br- (g), -337 k] mol -1.

A vapour at 22 atm and 5°C was allowed to expand adiabatically to a final pressure of 1:00 atm; the temperature fell by 10 K. Calculate the Joule- Thomson coefficient, u, at 5°C, assuming it remains constant over this temperature range.

Repeat Exercise 2.30(a) for argon, from an initial volume of 1.00 dm3 to 22.1 dm3 at 298 K.

The volume of a certain liquid varies with temperature as

V= V'{0.77 + 3.7 x 10^{-4}(T/K) + 1.52 X 10^{-6}(T/K) ^{2}}

The isothermal compressibility of lead at 293 K is 2.21 X 10-6 atm-1, Calculate the pressure that must be applied in order to increase its density by 0.08 per cent.

Given that μ = 1.11 K atm-I for carbon dioxide, calculate the value of its isothermal Joule- Thomson coefficient. Calculate the energy that must be supplied as heat to maintain constant temperature when 12.0 mol CO2 flows through a throttle in an isothermal Joule-Thomson experiment and the pressure drop is 55 atm.

A sample consisting of 1 mol of perfect gas atoms (for which CV•m = 3/2 R) is taken through the cycle shown in Fig. 2.34.

(a) Determine the temperature at the points 1, 2, and 3.

(b) Calculate q, w, ∆U, and ∆H for each step and for the overall cycle. If a numerical answer cannot be obtained from the information given, then write in +, -, 0, or? As appropriate

A sample consisting of2.0 mol CO2 occupies a fixed volume of 15.0 dm3 at 300 K. When it is supplied with 2.35 kJ of energy as heat its temperature increases to 341 K. Assume that CO2, is described by the van der Waals equation of state, and calculate w, ∆U, and ∆H

A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2 R is put through the following cycle:

(a) Constant-volume heating to twice its initial volume,

(b) Reversible, adiabatic expansion back to its initial temperature,

(c) Reversible isothermal compression back to 1.00 atm. Calculate q, w, ∆U, and ∆H for each step and overall.

(a) Constant-volume heating to twice its initial volume,

(b) Reversible, adiabatic expansion back to its initial temperature,

(c) Reversible isothermal compression back to 1.00 atm. Calculate q, w, ∆U, and ∆H for each step and overall.

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