Suppose you mix two volumes of water: 25.0 mL at 15°C and 35.0 mL at 68°C. What's the final temperature of the water? Assume the density of the water is 1.0 g/mL at both temperatures and the heat capacity of water is 4.184J/g°C.

If you add 10ml of hot water to 10ml of cold water and the change in tempature 8°c calculate how much energy is gained by the cold water

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)

Arrange the elements in order of increasing electronegativity. use the periodic table to you arrange the elements. p o k mg