A 2.4-cm-thick wood floor covers a 4.0m A container holds 1.1g of argon at a pre

Question

A 2.4-cm-thick wood floor covers a 4.0m

A container holds 1.1g of argon at a pressure of 8.5atm .How much heat is required to increase the temperature by 100 ? C at constant volume?How much will the temperature increase if this amount of heat energy is transferred to the gas at constant pressure? A 2.4-cm-thick wood floor covers a 4.0m5.5m room.The subfloor on which the flooring sits is at a temperature of 16.3 ? C , while the air in the room is at 19.3 ? C . What is the rate of heat conduction through the floor? Use 0.200 W/m?K for the thermal conductivity of wood. How many cubic millimeters (mm 3 ) are in 1L ?

Explanation / Answer

a)
Since no work is done in a constant volume process, the change of internal energy equals the heat transferred to the gas.
?U = Q
Assuming ideal gas behavior, the internal energy of the argon sample ideal gas is given by:
U = n?Cv?T
thus,
?U = n?Cv??T

The molar heat capacity at constant volume of a monatomic ideal gas like argon is:
Cv = (3/2)?R

The number of moles in the sample is
n = m/M = 1.1g / 39.948g/mol = 2.704

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