   Chapter 5, Problem 109SCQ

Chapter
Section
Textbook Problem

Suppose that an inch (2.54 cm) of rain falls over a square mile of ground (2.59 × 106 m2). (Density of water is 1.0 g/cm.) The enthalpy of vaporization of water at 25 °C is 44.0 kJ/mol. How much energy is transferred as heat to the surroundings from the condensation of water vapor in forming this quantity of liquid water? (The huge number tells you how much energy is “stored” in water vapor and why we think of storms as such great forces of energy in nature. It is interesting to compare this result with the energy given off, 4.2 × 106 kJ, when a ton of dynamite explodes.)

Interpretation Introduction

Interpretation: Heat energy transferred has to be identified. Compare the result with energy given out when dynamite explodes.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.

q=C×m×ΔT

Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity,ΔT= change in temperature.

Explanation

To calculate the volume

Area =1mi21×(1km)2(0.62137mi)2×(105cm)(1km)22 =2.59×1010cm2

1Inch=2.54cm

The volume of water =2

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