Question

(I) An ideal gas expands isothermally, performing\({\bf{4}}{\bf{.30 \times 1}}{{\bf{0}}^{\bf{3}}}\;{\bf{J}}\) of work in the process. Calculate (a) the change in internal energy of the gas, and (b) the heat absorbed during this expansion.

Short answer

(a) The change in internal energy is zero.

(b) The heat absorbed in the system is \(4.30 \times {10^3}\;{\rm{J}}\).

Step-by-step solution

Concepts

From the first law of thermodynamics,\(\Delta U = Q - W\).

For the isothermal process, the change in internal energy is\(\Delta U = 0\).

Given data

The work done in the process is \(W = 4.30 \times {10^3}\;{\rm{J}}\).

Calculation 

Part (a)

For the isothermal process, the change in internal energy is zero.

Part (b)

For the isothermal process,

\(\begin{array}{c}0 = Q - W\\Q = W\\Q = 4.30 \times {10^3}\;{\rm{J}}{\rm{.}}\end{array}\)

Hence, the absorbed heat in the system is \(4.30 \times {10^3}\;{\rm{J}}\).