vi. One mole of an ideal gas is compressed from 500 cm3 against a constant external pressure of 1.2 × 105 Pa. The work involved in the process is 36.0 J. Calculate the final volume. (200 cm3)
Given:
To find: Final volume (\(V_2\))
Formula: \(W = -P_{\text{ext}} \Delta V = -P_{\text{ext}} (V_2 - V_1)\)
Calculation:
Now, from the formula:
\[W = -P_{\text{ext}} \Delta V = -P_{\text{ext}} (V_2 - V_1)\]Therefore:
\[\frac{0.360 \, \text{dm}^3 \, \text{bar}}{1.2 \, \text{bar}} = -(V_2 - 0.5 \, \text{dm}^3)\]So:
\[0.3 \, \text{dm}^3 = -V_2 + 0.5 \, \text{dm}^3\]Thus:
\[V_2 = 0.2 \, \text{dm}^3 = 200 \, \text{cm}^3\]The final volume (\(V_2\)) is 200 cm3.
Chemical Thermodynamics Chapter 4 Chemistry Class 12 Textbook Solution