A 2.00-kg block of copper at 22.0°C is dropped into a large vessel of liquid nitrogen at 77.3 K. How many kilograms of nitrogenboil away by the time the copper reaches 77.3 K? (The specific heat of copper is 0.092 0 cal/g °C, and the latent heat ofvaporization of nitrogen is 48.0 cal/g.)kgNeed Help?Read ItWatch It

Answered: A 2.00-kg block of copper at 22.0°C is…

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

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A 2.00-kg block of copper at 22.0°C is dropped into a large vessel of liquid nitrogen at 77.3 K. How many kilograms of nitrogen
boil away by the time the copper reaches 77.3 K? (The specific heat of copper is 0.092 0 cal/g °C, and the latent heat of
vaporization of nitrogen is 48.0 cal/g.)
kg
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Expert Solution

Step 1

When a hot body is connected to a cold body then there occurs a transfer of heat between the two objects until here occurs a thermal equilibrium. The total heat amount gained by the cold body, as per the calorimetry principle, is equal to the heat amount lost by the hot body.

Now the formula to calculate the amount of heat lost by the copper is given by

$Q_{l o s t} = m c ∆ t$

where $m$ is the copper block's mass, $c$ is the specific heat and $∆ t$ is the temperature change.

The initial temperature of the block is

$T_{i} = 22 . 0^{\circ} C$

Final temperature of the block is

$T_{f} = {(77.3 - 273.15)}^{\circ} C = - 195 . 85^{\circ} C$

As it can be seen that $T_{i} > T_{f}$ thus the temperature of the block drops.

Now the formula to calculate the change in temperature is given by

$∆ T = T_{i} - T_{f}$

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