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.)

Name: suppose that 095 g of water condenses on a 750 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 2
Uploaded: 2019-11-12T15:07:49-08:00
Duration: 1 min 5 s
Channel: Lizabeth Tumminello
Description: suppose that 095 g of water condenses on a 750 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 2

          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.)

Added by Richard L.

Chemistry A Molecular Approach

Nivaldo J. Tro 4th Edition

Chapter 11

Instant Answer

Solved by Expert Lizabeth Tumminello

11/12/2019

Step 1

To find the number of moles of water, use the formula: \[ \text{moles} = \frac{\text{mass}}{\text{molar mass}} \] Given that the mass of water is 0.95 g and the molar mass of water (H₂O) is approximately 18.015 g/mol, the calculation is: \[ \text{moles of water} = 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 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.)