Methanol as a fuel for internal combustion engines

Abstract

Transportation of people and goods largely relies on the use of fossil hydrocarbons, contributing to global warming and problems with local air quality. There are a number of alternatives to fossil fuels that can avoid a net carbon emission and can also decrease pollutant emissions. However, many have significant difficulty in competing with fossil fuels due to either limited availability, limited energy density, high cost, or a combination of these. Methanol (CH 3 OH) is one of these alternatives, which was demonstrated in large fleet trials during the 1980s and 1990s, and is currently again being introduced in various places and applications. It can be produced from fossil fuels, but also from biomass and from renewable energy sources in carbon capture and utilization schemes. It can be used in pure form or as a blend component, in internal combustion engines (ICEs) or in direct methanol fuel cells (DMFCs). These features added to the fact it is a liquid fuel, making it an efficient way of storing and distributing energy, make it stand out as one of the most attractive scalable alternatives. This review focuses on the use of methanol as a pure fuel or blend component for ICEs. First, we introduce methanol historically, briefly introduce the various methods for its production, and summarize health and safety of using methanol as a fuel. Then, we focus on its use as a fuel for ICEs. The current data on the physical and chemical properties relevant for ICEs are reviewed, highlighting the differences with fuels such as ethanol and gasoline. These are then related to the research reported on the behaviour of methanol and methanol blends in spark ignition and compression ignition engines. Many of the properties of methanol that are significantly different from those of for example gasoline (such as its high heat of vaporization) lead to advantages as well as challenges. Both are extensively discussed. Methanol's performance, in terms of power output, peak and part load efficiency, and emissions formation is summarized, for so-called flex-fuel engines

The Electron Impact Ionization Cross Sections of Methanol, Ethanol and 1-Propanol

“…where h(Q) is same as given by Equation (8). Using Equations (5) and (7) with Equation (2), Khare and his associate [17] obtained the total ionization cross section due to longitudinal interaction in their BEB model given by [17] (omitting the subscript j)…”

“…We took E + I + U = E at relativistic energies. M 2 is calculated from Equation 4, using the expression of the COOS, given by Equation (5). Calculated values of M 2 and C RP are tabulated in Table 2.…”

“…Plasma is created during the combustion of biofuels. Plasma modelling is required to make the theoretical model of car engines and the ionization cross sections may be used as an input parameter [4][5][6]. Furthermore, alcohols are detected in the interstellar space medium and also in the atmosphere of planets in the solar system.…”

Exhaust Emissions and Physicochemical Properties of n-Butanol/Diesel Blends with 2-Ethylhexyl Nitrate (EHN) or Hydrotreated Used Cooking Oil (HUCO) as Cetane Improvers

“…Ethanol, in particular, is already widely and successfully used in spark-ignition engines, while extensive research was also conducted for its potential implementation in diesel engines [5,[28][29][30]. Methanol, studied and tested in the past, was recently reintroduced in various places and applications [31]. Furthermore, n-butanol is considered more compatible for use in blends with ULSD because it does not suffer from miscibility issues, and its physicochemical properties are somewhat closer to those of diesel fuel [5,24,32].…”

Decomposition of Methanol on Supported Pd–Au Catalyst for Recovery of Unused Waste Heat at Low Temperature

“…Methanol decomposition according to the following equation is an endothermic reaction which proceeds at temperatures higher than 423 K from the chemical equilibrium. CH3OH = CO + 2H2 H = 95.3 kJ mol G = 3.2 kJ mol at 423 K (1) This reaction is simple, however, is more endothermic than the steam reforming reaction as follows 2),3) ; CH3OH + H2O = CO2 + 3H2 H = 54.8 kJ mol G = 26.7 kJ mol at 423 K (2) In addition, CH3OH is now considered as promising biofuel for automobiles 4) , through simple oxidation as shown in the Eq. 3 Total H = 769.6 kJ mol G = 691.9 kJ mol at 423 K (6) Therefore, this reaction is considered suitable for application to automobiles 5) .…”