# Lenoir cycle: Wikis

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# Encyclopedia

Updated live from Wikipedia, last check: May 21, 2013 21:39 UTC (46 seconds ago)

The Lenoir cycle is an idealized thermodynamic cycle often used to model a pulse jet engine. It is based on the operation of an engine patented by Jean Joseph Etienne Lenoir in 1860. This engine is often thought of as the first commercially produced internal combustion engine. The absence of any compression process in the design leads to lower thermal efficiencies than the more well known Otto cycle and Diesel cycle.

In the cycle, an ideal gas undergoes

1-2: Constant volume (isochoric) heat addition;
2-3: Isentropic expansion;
3-1: Constant pressure (isobaric) heat rejection—compression to the volume at the start of the cycle.

The expansion process is isentropic and hence involves no heat interaction. Energy is absorbed as heat during the isochoric heating and rejected as work during the isentropic expansion. Waste heat is rejected during the isobaric cooling which consumes some work.

## Constant volume heat addition (1-2)

In the ideal gas version of the traditional Lenoir cycle, the first stage (1-2) involves the addition of heat in a constant volume manner. This results in the following for the first law of thermodynamics: ${}_1Q_2 = mc_v \left( {T_2 - T_1 } \right)$

There is no work during the process because the volume is held constant: ${}_1W_2 = \int\limits_1^2 {pdV} = 0$

and from the definition of constant volume specific heats for an ideal gas: $c_v = \frac{R}{{\gamma - 1}}$

Where R is the ideal gas constant and γ is the ratio of specific heats (approximately 287 J/(kg·K) and 1.4 for air respectively). The pressure after the heat addition can be calculated from the ideal gas law: p2V2 = RT2

## Isentropic expansion (2-3)

The second stage (2-3) involves a reversible adiabatic expansion of the fluid back to its original pressure. It can be determined for an isentropic process that the second law of thermodynamics results in the following: $\frac{{T_2 }}{{T_3 }} = \left( {\frac{{p_2 }}{{p_3 }}} \right)^{{\textstyle{{\gamma - 1} \over \gamma }}} = \left( {\frac{{V_3 }}{{V_2 }}} \right)^{\gamma - 1}$

Where p3 = p1 for this specific cycle. The first law of thermodynamics results in the following for this expansion process: ${}_2W_3 = mc_v \left( {T_2 - T_3 } \right)$ because for an adiabatic process: 2Q3 = 0

## Constant pressure heat rejection (3-1)

The final stage (3-1) involves a constant pressure heat rejection back to the original state. From the first law of thermodynamics we find: 3Q13W1 = U1U3.

From the definition of work: ${}_3W_1 = \int\limits_3^1 {pdV} = p_1 \left( {V_1 - V_3 } \right)$, we recover the following for the heat rejected during this process: ${}_3Q_1 = \left( {U_1 + p_1 V_1 } \right) - \left( {U_3 + p_3 V_3 } \right) = H_1 - H_3$.

As a result, we can determine the heat rejected as follows: ${}_3Q_1 = mc_p \left( {T_1 - T_3 } \right)$ from the definition of constant pressure specific heats for an ideal gas: $c_p = \frac{{\gamma R}} {{\gamma - 1}}$.

The overall efficiency of the cycle is determined by the total work over the heat input, which for a Lenoir cycle equals $\eta _{th} = \frac{{{}_2W_3 + {}_3W_1 }} {{{}_1Q_2 }}$. Note that we gain work during the expansion process but lose some during the heat rejection process.