When 3.0 mole of an ideal diatomic gas is heated and compressed simultaneously from 300K, 1.0 atm to 400K and 5.0atm, the change in entropy is (Use C_(P) = (7)/(2)R for the gas)
Calculate the Delta H for the isothermal reversible expansion of 1 mole of an ideal gas from initial pressure of 1.0 bar to a final pressure 0.1 bar at a constant temperature at 273K.
Assuming that, water vapour is an ideal gas the internal energy (Delta U) when 1 mol of water is vapourised at 1 bar pressure and 100^(@)C (given : molar enthalpy of vaporisation of water at 1 bar and 373 K = 41 kJ mol^(-1) and R = 8.3 J K^(-1) mol^(-1) )) will be
Calculate the free energy change in kJ when 1 mole of NaCl is dissolved in water at 298 K, Given a) U of NaCl (U = lattice energy) = 778 kJ "mole"^(-1) b) Hydration energy of NaCl = -774.3 kJ "mole"^(-1) (c) Entropy change at 298K = 43 "mole"^(-1)
The Henry's constant for solubility of N_(2) gas in water at 298K is 1.0xx10^(5) atm. The mole fraction of N_(2) in air is 0.8 . The number of moles of N_(2) from air dissolved in 10 moles of water at 298K and 5 atm pressure is :
The molar heat capacity at constant volume of a system is 12.41J. mol^(-1) . In an adiabatic expansion the temperature of one mole of that gas falls from 298K to 288K. Calculate the work done by the gas.
If bar(i), bar(j), bar(k) are unit vectors along the positive directions of the coordinate axes, then shown that the four points 4 bar(i) + 5 bar(j) + bar(k), - bar(j) - bar(k), 3 bar(i) +9 bar(j) + 4 bar(k) and - 4 bar(i) + 4 bar(j) + 4 bar( k) are coplanar
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
