Complete combustion of 1 mol of propane (C3H8) liberates -2044 kJ/mol: C3H8(g) + 5O2 → 3 CO2(g) + 4H2O
Using this information together with the standard enthalpies of formation given below, calculate the standard enthalpy of formation of propane.
CO2(g)= -393.5 kJ/mol
O2 = 0 kJ/mol
H2O = -284 kJ/mol

A) -568 kJ/mol
B) -418 kJ/mol
C) -272.5 kJ/mol
D) 150 kJ/mol

A50.0g sample of liquid water at 0.0 c ends up as ice at -20.0 c. how much energy is involved in this change?

Many ionic compounds and a few highly polar covalent compounds are because they completely ionize in water to create a solution filled with charged ions that can conduct an electric current.

The lattice enthalpy (formation of ionic solid from ions in the gas phase) for agcl(s) is -916 kj/mol and the hydration enthalpy (dissolution of gaseous ions into water) is -850 kj/mol. how much heat (in joules) is involved in forming 1l of saturated agcl solution (1.8 × 10-4 g / 100 ml water) by dissolving agcl(s)? assume solution volume does not change much upon dissolution. the equations are given below. ag+(g) + cl−(g) æ agcl(s)