A 2.375-g sample of impure Mn2(CO3)5 is decomposed with heat. 64.33 mL of CO2 is collected over water at a temperature of 40.00oC. The gas is collected at an atmospheric pressure of 755 torr. Water has a vapor pressure of 37 torr at 40.00oC. What is the % Mn2(CO3)5 in the original impure sample? Mn2(CO3)5 → Mn2O5 + 5 CO2

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)