Question

Asked Sep 17, 2019

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A house has well-insulated walls. It contains a volume of 90 m^{3} of air at 315 K.

(a) Consider heating it at constant pressure. Calculate the energy required to increase the temperature of this diatomic ideal gas by 1.4°C.

(b) If this energy could be used to lift an object of mass *m* through a height of 2.3 m, what is the value of *m*?

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Step 1

Solution:

Given that the air is contained inside a house, the Pressure *P* of the gas can be taken equal to the atmospheric pressure.

The Ideal gas Equation is used for calculating the number of moles *n *of a diatomic gas (air) within the house.

The ideal gas equation is given by,

Step 2

Here *V* is the volume of the diatomic gas(air) contained inside the house, *R* is the gas constant , *n* is the number of moles of the diatomic gas (air) and *T* is the initial Temperature of the diatomic gas.

Substitute 1.013 x 10^{5 }N / m^{2} for *P*, 90 m^{3} for *V,* (air), 8.314 J/ mole.K for *R*, 315 K for *T * and solve for *n* as,

Step 3

The first law of thermodynamics for Work done on ...

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