Question
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.)
Step 1
The molar mass of water is approximately 18 g/mol. Therefore, the number of moles of water is given by: \[n = \frac{m}{M} = \frac{0.95 \, \text{g}}{18 \, \text{g/mol}} = 0.053 \, \text{mol}\] Show more…
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Suppose that 0.95 g of water condenses on a 75.0 -g block of iron that is initially at $22^{\circ} \mathrm{C}$ . If the heat released during condensation goes only to warming the iron block, what is the final temperature ( in $^{\circ} \mathrm{C} )$ of the iron block? (Assume a constant enthalpy of vaporization for water of 44.0 $\mathrm{kJ} / \mathrm{mol.}$ .
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