# Question

A 1.50-mole sample of an ideal gas is allowed to expand adiabatically and reversibly to twice its original volume. In the expansion the temperature dropped from 296 K to 239 K. Calculate ΔE and ΔH for the gas expansion.

## Answer to relevant Questions

Consider 1.00 mole of CO2(g) at 300. K and 5.00 atm. The gas expands until the final pressure is 1.00 atm. For each of the following conditions describing the expansion, calculate q, w, and ΔE. Cp for CO2 is 37.1 J K-1 ...The enthalpy of vaporization of chloroform (CHCl3) is 31.4 kJ/ mol at its boiling point (61.7oC). determine ΔSsys, ΔSsurr, and ΔSuniv when 1.00 mole of chloroform is vaporized at 61.7oC and 1.00 atm. Using the following data, calculate the value of Ksp for Ba(NO3)2, one of the least soluble of the common nitrate salts. Consider the isothermal expansion of 1.00 mole of ideal gas at 27oC. The volume increases from 30.0 L to 40.0 L. Calculate q, w, ΔE, ΔH, ΔS, and ΔG for two situations: a. a free expansion b. a reversible expansion Using data from Appendix 4, calculate ΔHo, ΔGo, and K (at 298 K) for the production of ozone from oxygen: 3O2(g) ⇌ 2O3(g) At 30 km above the surface of the earth, the temperature is about 230. K and the partial pressure ...Post your question

0