Thermodynamics | First Law of Thermodynamics#
First Law of Thermodynamics#
- Whenever the state of a system changes, there will be change in its internal energy.
- This change in its internal energy can be done by two ways: (a) by doing work on the system or work is done by the system (b) by supplying heat to the system or heat is released by the system.
- This is known as First Law of Thermodynamics. It is based on energy conservation principle.
- Mathematically, we can express first law of thermodynamics as:
\[ΔU = q + W\]
Question#
A gas contained in a cylinder fitted with a frictionless piston expands against a constant external pressure of 1 atm from volume 4 L to 14 L. In doing so, it absorbs 800 J from surrounding. Calculate the change in internal energy of the system.
\[W = - \int\limits_{V_1}^{V_2} P_{ext}dV\]
Since Pext is constant, we can write this as:
\[W = -P_{ext} (V_2 - V_1)\]
\[W = -1 (14 - 4)\]
\[W = -10\ atm L \]
\[W = -10 \times 101.3\ J\ (Since,\ 1\ atm\ L = 101.3\ J)\]
\[W = -1013\ J\]
Now, calculating ΔU from first law of thermodynamics:
\[ΔU = q + W\]
\[ΔU = 800\ J + (-1013)\ J\]
\[ΔU = -213\ J\]
- Please note that we have used heat absorbed by the system as +800 J in the question as per sign convention.