Molecular hydrogen gas having a mass of 6.44 g at 26.0^∘ C is heated until its volume doubles w

step 1 We have to find the value of work done for nitrogen gas having mass 6 .44 gram at 26 degrees Cel

Molecular hydrogen gas having a mass of 6.44 g at 26.0^∘ C...

Molecular hydrogen gas having a mass of $6.44 \mathrm{~g}$ at $26.0^{\circ} \mathrm{C}$ is heated until its volume doubles while it is held at a constant pressure. How much work was done by the gas? [Hint: Take it to be an ideal gas.]

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Key Concepts

Isobaric Process

An isobaric process is a thermodynamic process in which the pressure remains constant while the volume and temperature can change. In such a process, the work done by a gas is directly related to the change in volume, making it straightforward to calculate using the product of the constant pressure and the change in volume.

Ideal Gas Law

The ideal gas law is a fundamental relation in thermodynamics expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin. This law describes how the state variables of an ideal gas are interconnected and provides the basis for calculating changes in the gas’s properties during various processes.

Thermodynamic Work

Thermodynamic work refers to the energy transferred by a system when it undergoes a change in volume against an external pressure. In the context of an isobaric process, the work done by the gas is calculated with the formula W = P?V, linking the concepts of pressure and volume change to energy transfer.

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