Suppose that 0.95 g of water condenses on a 75.0 g block of iron that is initially at 22 °c. if the heat released during condensation is used only to warm the iron block, what is the final temperature (in °c) of the iron block? (assume a constant enthalpy of vaporization for water of 44.0 kj/mol.)

First to find how much energy was transferred;

(0.88 g H2O) x (1 mol H2O / 18.02 g H2O) x (44.0 kJ / mol)

= 2.3 kJ

For the next step you must know that the specific heat of iron is 0.449 J / (g) (K).

((g) (K) / 0.449 J) x (2.1 kJ) x (1000 J / kJ) x (1 / 75.0 g)

= 68 K

This means that the block gained enough energy to raise its temperature by 68 K.

So, the final temperature is 363 K or 89.85 degrees Celsius.