Reference no: EM132610697
Q1. Test the cyclic rule for the equation, (p + a/Vm2)(Vm) = RT
Q2. Mathematically show that the magnitude of the work involved in a reversible expansion of an ideal gas from volume V1 to V2 is larger than the corresponding work involved in an irreversible expansion against a constant pressure of p2.
Q3. Calculate the ?U and qV for the transformation of 1 mol of helium at constant volume from 250C to 450C; Cv = 3/2R.
Q4. 1 mole of an ideal gas undergoes reversible isothermal expansion from an initial volume of V to final volume 10 V and does 10 KJ of work. If the initial pressure was 107 Pa then the value of V is?
Q5. The value of ?U for the transformation of one mole of an ideal gas from 270C and 1 atm to 3270C and 1 atm is? (given that Cp= 20.9 + 0.042T J/K-mole)
Q6. A mass of mercury at standard atmospheric pressure and a temperature of 15 deg C is kept at constant volume. If the temperature is raised to 25 deg C, what will be the final pressure? Given that thermal expansibility (α) 1.81*10-4 k-1 and thermal compressibility (β) 4.01*10-11 Pa-1.
Q7. Calculate πT and Cp - CV for van der Waals gas.
Q8. Starting from total differential of H, show that (∂H/∂T )V = Cp(1 - αμJT /κ) .
Q9. Assign the following reaction whether exothermic or endothermic----
a. NaOH (aq) + HCl (aq) --> NaCl + H2O
b. C (s) + H2O (l) --> CO (g) + H2 (g)
c. 6CO2 + 6H2O > C6H12O6 + 6O2
Q10. A 0.138 g sample of solid Mg (M = 24.30 g/mol) is burned in a bomb calorimeter that has a heat capacity of 1.77 kJ ºC-1. The calorimeter contains 300 mL of water (density = 1 g/mL) and its temperature is raised by 1.126 ºC. Calculate the enthalpy of combustion of Mg at 298K.
Q11. Given the following ΔH° 298 /(kJ/mol) values,
4NH3(g) + 5O2(g) → 4NO (g) + 6H2O (l) ΔH =- 1170
2NO (g) + O2(g) → 2NO2(g) ΔH =- 114
3NO2 (g) + H2O (l) → 2HNO3(l) + NO (g) ΔH =- 72
find ΔH° 298 for NH3(g) + O2(g) → HNO3(l) + H2O