The Different Roles of Fire Professionals and Their Importance to Fire Safety - Essay Example

FIRE PROFESSIONALS Student’s Name Institutional Affiliation Date Section A 1. In 1000 words discuss the different roles of fire professionals and their importance to fire safety. Firefighting is one of the most important services required in a community. Organizations that deal with fire control should be spread evenly in places that have a high risk of fire breakout. There are different professions with varied responsibilities in a fire department that enable effective operations. The professions in firefighting include chief fire officer, assistant chief fire officer, area manager, group manager, station manager, crew manager, watch manager, and the firefighter. The Chief Fire Officer performs several administrative, supervisory, and technical works in organizing, planning, implementing, and directing fire suppression, prevention, and emergency medical services that minimize or prevent the loss of life (New Hampton, 2008). Fire cases are risky and can involve medical emergencies due to suffocation, burns, or falling due to panic. The Chief Fire Officer coordinates, evaluates, and supervises fire and emergency medical services operations (New Hampton, 2008). Firefighting departments must have emergency medical response teams that attend to emergencies from their operational environment before the patients reach the hospital. He or she also establishes procedures and policies for emergency medical services and firefighting. It is important to have the right procedures to avoid risking the lives of either the firefighters or victims of a fire incident. The officer also reviews the performance and effectiveness of the department, and recommends implementation of innovative technology (New Hampton, 2008). Technology changes as people try new and more efficient methods of firefighting aimed at improving the efficiency of the practice and lowering the risks associated with fighting fire. He or she trains personnel in all features of the job (New Hampton, 2008). It is essential for the professionals in firefighting departments to have enough knowledge of their respective roles. It ensures that they work effectively and apply professional approaches in making decisions concerning fires. The Chief Fire Officer attends meetings and conferences to know the current trends in the practice. He or she also takes command of major fire incidents. The Assistant Chief Fire Officer takes the responsibilities of the Chief Fire Officer whenever he or she is absent and ensures that all operations run efficiently. Another important role is that of an Area Manager, who is responsible for daily management of an area of the policy or operation of the fire brigade. He or she selects the required personnel and supports and monitors people to resolve operational incidents (South Yorkshire Fire and Rescue, 2005). People have different talents and understanding of processes. They also have varied personality that can influence their response to fire situations. Area Manager ensures that the firefighting personnel are well-equipped for their work. He or she then guides them towards solving operational incidents efficiently so that they learn easily and know how to respond to similar incidents. The Area Manager also manages the performance of individuals and teams to attain objectives (South Yorkshire Fire and Rescue, 2005). Firefighters work in teams, and it is important for every member to be professional and skillful so as to enhance the performance of the group. Group Manager manages a group of fire stations or groups of activities in a particular policy area. The number of fire stations varies based on the availability of sufficient officers and the risk of fires in the region. He or she deals with other responsibilities that incorporate organizational responsibilities and deal with firefighters under his or her area of operation. Some of the responsibilities include implementing quality assurance systems, monitoring agreement with quality systems, developing teams and advising on the implementation of policies (South Yorkshire Fire and Rescue, 2005). Quality assurance ensures that the services of a fire brigade meet the standard quality necessary to provide good fire control services. It is, therefore, essential that the Group Managers implement quality assurance systems and frequently monitor the systems to ensure they comply with current practices. They develop teams that are well-equipped to overcome the challenges associated with firefighting. Since they have a leadership role, they provide advice on policies based on their experience and observation of various activities. The main responsibility of Station Managers is to manage a fire station and coordinate activities around the station. The Station Manager ensures effective utilization of resources, implements, and plans activities to meet the needs of service delivery, and provides information that helps in decision-making (South Yorkshire Fire and Rescue, 2005). Resources include everything that goes into firefighting such as fuel for fire trucks, the fire trucks, and the material used in extinguishing fire. Since they are based at a fire station, they receive information about fires at different places and give information that aid in making firefighting decisions based on the magnitude of the problems. They plan firefighting activities to ensure the team offers a good service to customers. The Watch Managers and Crew Managers have some similarity in their responsibilities. They manage information that requires action, investigate and provide reports on events, and are responsible for the performance of their teams (South Yorkshire Fire and Rescue, 2005). They obtain, store and provide resources required in service delivery. However, Watch Managers keep watch at large fire stations while Crew Managers watch smaller stations and the team associated with a fire appliance. The latter also gets involved in firefighting and attends fire occurrences as an officer in control of an appliance. Another most important person among the fire professionals is the firefighter. A firefighter is responsible for day-to-day fire safety and firefighting work. Firefighters coordinate responses to help with resolving a fire event, maintain readiness and reliability of equipment that help in fire control, help colleagues to develop, drive and redeploy vehicles used in fire service, and use and maintain databases (South Yorkshire Fire and Rescue, 2005). They coordinate themselves to control fires in various situations. The experienced firefighters develop their colleagues to ensure they gain experience and contribute to an efficient team. The readiness of the firefighting equipment leads to quick response to fire events and early control of the situation. It is important to define the roles of every department in a fire brigade to ease coordination and improve efficiency of services. 2. In 500 words discuss the term “flame” and identify the different categories of flame. The gaseous and visible part of the fire is referred to as flame. A flame is produced once the fire has started. As a result, a flame can only be seen where there is a fire. The flame is visible as a result of an extremely exothermic reaction taking place within a confined zone enclosing the flame. Flames are of different colours with varying temperatures depending on the type of fuel burned. As the fire develops, part of the fuel vaporizes and mix with air (oxygen) for a continuous combustion. The flame is maintained by subsequent exothermic reaction that dissipate heat, which in turn vaporize more fuel for further consumption. The amount of heat released dictates the temperature of the flame, and the energy of the flame emit light from the flame. The average quantity of the energy released by the flame increases with the combustion temperature. The flame colour, especially from hydrocarbon fuels, depends on the quantity of oxygen supplied for combustion and the ratio of fuel oxygen pre-mixing. Both factors determine the rate of combustion, which results in different temperatures of flame and heat of reaction leading to different colour hues. Oxygen supply controls the extent of fuel combustion. With adequate fuel supply, sufficient supply of oxygen ensures fuel molecules are burned to near completion producing a blue colour. The blue region is the hottest part of the flame. When the amount of oxygen supplied is insufficient, the fuel combustion is incomplete producing a yellow flame. The yellow flame indicates the presence of unburnt fuel particles as a result of inadequate supply of oxygen. Therefore, a flame comprises unburned, preheat, reaction, and burned gas (University of Sheffield, 2000). Flames are categorized depending on several factors resulting in several types of flames across the world. However, flames are classified into two primary types; premixed flame and diffused flame (University of Sheffield 2000). Majority of flames falls under this classification. The extent of fuel-air mixing determines, which category a flame falls in. Premixed flames involve the use of fuel premixed with air (oxygen) before being introduced into the burning chamber. Premixed flames are further divided into laminar and turbulent premixed flames. In a laminar premixed flame, the premixed fuel and air flow into the burning zone in a streamline producing a smooth burning (University of Sheffield, 2000). A Bunsen burner flame is an example of a laminar premixed flame, the air and gas are mixed, channeled through the pipe to the top burning spot. In turbulent premixed flames, fuel and air are premixed in some devices before the combustion chamber. The examples of turbulent premixed flames include flames from furnaces and boilers. In diffused flames, fuel and air reach the burning chamber unmixed. Diffused flame is also divided into laminar and turbulent diffused flames (University of Sheffield, 2000). In a laminar diffused flames, fuel and air do not mix until they are introduced to the burning zone. The supply of both fuel and air (oxygen) are in parallel before ignition. A burning candle is an example of a laminar diffused flame. On the other hand, turbulent diffused flames comprise the practical (University of Sheffield, 2000). 3. In 200 words explain the similarities and differences between fires and explosions. Most people often find it difficult to point the differences between fire and explosion because, in one way or the other, one may lead to another. Fire, in the presence of explosive materials, may cause an explosion while explosion can also lead to fire as well. However, there are distinct differences and similarities between fire and explosion. An explosion involves quick reactions that lead shock waves. There are no shock waves with fire. An explosion can only occur when exposed to shock or heat, while fire does start when only exposed to heat in the presence of fuel-air mixture. While an explosion needs detonation to occur, fire does not require a detonator. In addition to the differences, fire and explosion do have some similarities. Fire and explosion need an oxygen source to enable the fuel source to burn or combust. Oxygen supports burning of any fuel type. In addition, both the fire and explosion require a fuel source to start or detonate respectively. In the absence of fuel, there is no burning. The fire and explosion dissipate some heat energy and create light as well. Both fire and explosion do have a diverse effect on the environment they occur. Fire can consume anything in its path while explosion demolishes structures such buildings and landscapes. 4. In 500 discuss the different sources of ignition and common causes of fire. A fire needs a source of ignition in the presence of fuel and oxygen to start. A fire will not start in the absence of any of the three requirements. In fire safety, cutting out the source of ignition, fuel or oxygen will prevent fires from starting. Ignition can occur in two different ways, especially for the hydrocarbons. First, a fire will start when an external source of ignition has sufficient energy to ignite a fuel-oxygen mixture. Secondly, a fuel-oxygen mixture will auto-ignite at high temperatures above that of auto-ignition. In general, the ignition sources include hot work, static electricity, hot surfaces, electric arcs and sparks, pyrophoric iron sulphides, pressure-compression ignition, friction and mechanical sparks, sudden decompression, and catalysts (University of Calgary, 2010). Hot work Any operation that produces sufficient energy from a flame or any other sources of ignition to ignite flammable materials can be referred to as hot work. Such activities may include cutting, welding, drilling, welding, brazing, chipping, and soldering, which are capable of creating sparks or high temperatures (University of Calgary, 2010). These activities, when not handled with care, can become a dangerous cause of a fire. Static electricity Static electricity is another common source of ignition. When materials or equipments are not properly grounded, the positive and negative electrical charges may build up to the point of discharging static arcs. Static arcs can easily ignite flammable vapours within its vicinity. Hot surfaces Hot surfaces are other potential sources of ignition. Hot surfaces above the auto-ignition temperature of a flammable material may ignite such material. However, auto-ignition from hot surfaces is minimal due to environmental conditions that may make it difficult for a surface to attain extreme temperatures capable of auto-ignition. Electric arcs and sparks Sparks are electrons discharged from a material, and they are usually energy rich. On the other hand, an electric arc is generated when two conducting surfaces are in proximity and a continuous flow of electrons trying to bridge the gap between them (University of Calgary, 2010). However, an arc or spark can ignite a fuel-air mixture when they dissipate enough energy. Pressure (Compression ignition) Compression of vapours increases both the pressure and the temperature of the container and heat is transferred. Rapid compression may increase the temperature of the system such that the heat loss to the environment is negligible and such high internal temperature may ignite a fuel-air mixture in its reach. Catalysts Catalysts dictate the rate of reaction. In the presence of a catalyst, a chemical reaction may become rapid and violent, increasing the temperatures leading to ignition of the fuel-air mixture source. There are several causes of fire and all the above the mentioned sources of ignition are also fire causes. The first main cause of the fire is human error or mistakes in handling fire hazard materials or activities. Any source of flames such as candles or any burning material can easily start a fire when not managed well. Chemical and gases are high potential causes of fire if safety precautions are not adhered to and followed. On the bottom line, accidents, human error, and arson fire setting are the major causes of fire. Section B 1. Convert the following temperatures into Kelvin: Converting degree Celsius into Kelvin requires adding 273.15K to a given degree Celsius a) 0°C 0oC=273.5+0=273.5K b) -150°C -150oC=-150+273.5=123.5K c) 640°C 640oC=640+273.5=913.5K d) -20°C -20oC=-20+273.5=253.5K 2. How many moles of carbon are in 150.0 g? First, the mass of one carbon molecule (C) and its subsequent number of moles, which is one, are determined. The resultant values are then compared to the given mass (150.0g). The molecular mass of carbon (12g) and is one mole (1 mole). The number of moles in a given mass is computed by the formula: Number of moles=Mass of a substance (M)/Molecular mass of the substance (MM) Therefore, 150.0g of carbon gives; =150/12= 12.5 moles 3. Balance the following equations: In balancing chemical equations, number of the same molecules on both sides of equations must be equal. a) H3PO4 + NH4OH → H2O + (NH4)3PO4 First, there are seven H molecules on the left-hand side and 14 on the right-hand side. b) V2O5 + Ca → CaO + V To balance O molecules on both sides, 5 is placed before CaO to give 5CaO. Now there must be 5Ca on the left-hand side. On the right-hand side, there must be 2V for the equation to balance. Therefore, a balanced equation is: V2O5 + 5Ca → 5CaO + 2V c) BN + F2 → BF3 + N2 There must be two N molecules on the left-hand side (2BN) for it to balance. After balancing N molecules, two B molecules result on the left-hand side of the equation, which balances with 2BF3. Hence, F molecules on the left-hand side are 3F2 giving a balanced equation as: 2BN + 3F2 → 2BF3 + N2 d) 2C15H26 + 43O2→ 30CO2 +26H2O The equation must have 26 water molecules (26H2O) and 2C15H26 for H molecules to balance on both sides of the equation. 30CO2 will balance the number of C molecules in the equation. Now, the water and carbon dioxide molecules on the left-hand side of the equation give a sum of 86 molecules of Oxygen (O) and for it to balance on both sides, there must be 43O2 in the equation. A balanced equation is given as: 2C15H26 + 43O2→ 30CO2 +26H2O e) Ca + N2 → Ca3N2 In this equation, only Ca molecules are not balanced. It would be balanced with 3Ca. Thus, a balanced equation is given as: 3Ca + N2 → Ca3N2 4. Ammonia and oxygen react to form nitrogen and water: 4NH3 + 3O2 → 2N2 + 6H2O a) How many grams of O2 are needed to react with 8.0 moles of NH3? From the reaction equation, 4.0 moles of NH3 are needed to react with 3.0 moles of O2. Therefore, 8.0 moles of NH3 would require 8/4*3=6.0 moles of O2 to react. The molecular mass of O2 is 32.0g. 6 moles of O2 give 6*32=192.0g Hence, 8.0 moles of NH3 would require 192.0g of O2 to react. b) How many grams of N2 can be produced when 6.50 grams of O2 reacts? From the equation, production of 2.0 moles of N2 requires 3 moles of O2. Number of moles of a substance=mass of the substance/molecular mass of the substance Therefore, 6.50g of O2 give 6.5/32=0.203 moles The number of N2 moles produced by 0.203 moles of O2 =0.203*2/3=0.135 moles Mass=No. Of moles *Molecular mass=0.135*28= 3.78 g of N2 will be produced by reacting 6.50 grams of O2. c) How many grams of water can be formed from the reaction of 34 g of NH3? Similarly, the equation requires 4.0 moles of NH3 to produce 6.0 moles of water (H2O). The molecular mass of NH3 is 17.0g, and the mass of 4 moles would be 17*4=68.0g. The molecular mass of water is 14.0g, and the mass of 6 moles would be 14*6=84.0g. 34g of NH3 will react to form 34/68*84=42.0g of water 5. Using the Ideal Gas Law, solve the following problems: (use 0.08206 L atm mol¯1 K¯1 for the gas constant). The Ideal Gas Law formula is given as PV=nRT (Nave, 2015a) Where P=pressure in the atmosphere, V=volume in liters, n=number of moles, R=gas constant (given), and T=temperature in Kelvin. a) Determine the volume of occupied by 3.34 grams of carbon dioxide gas at STP. At STP, Pressure is 1 atm and the temperature is 273.15K. Number of moles in 3.4g carbon dioxide Moles=Mass/Molecular mass=3.4/44=0.077 The volume of carbon dioxide occupied by 0.077 moles V=nRT/P=0.077*0.08206*273.15/1=1.726L b) A sample of argon gas at STP occupies 46.2 litres. Determine the number of moles of argon and the mass in the sample. First, the number of moles of Argon occupying 46.2 litres is determined. n=PV/RT = (1*46.2)/ (0.08206*273.15) =2.061 moles The molecular mass of argon gas is 40.0 g. The mass of the gas in 2.061 moles= 2.061*40= 82.44 g. c) At what temperature will 0.654 moles of neon gas occupy 12.30 litres at 1.95 atmospheres? T=PV/nR=12.3*1.95/ (0.654*0.08206) =446.9K d) A 30.6 g sample of gas occupies 22.414 L at STP. What is the molecular weight of this gas? n=PV/RT=1*22.414/ (273.15*0.08206) =1.0 mole. At STP, 1 mole of substance occupies 22.414 L at 1 atm and 273.15K. Consequently, the molecular weight of the sample gas is 30.6 g. 6. How many joules of heat are needed to raise the temperature of 10.0g of aluminium from 22°C to 55°C, if the specific heat of aluminium is 0.90J/g°C? The formula for the specific heat capacities is given by Q=MCp∆T (Nave, 2015b) Where, Q=heat dissipated or absorbed by the substance M=mass of the substance, Cp=specific heat of the substance, ∆T=Temperature change on the substance The amount of heat needed as per the question above determined as Q=10*0. 90* (55-22) =10*0. 9*33=297J. 7. A pan 200mm diameter pan is placed on a stove to boil some water. The thickness of the bottom of the pan is 7.5mm and the inner surface temperature of the bottom of the pan is 150°C. Determine the outer surface temperature of the pan is the pan was a) aluminium and b) copper. Assume one-dimensional, steady state conduction through the bottom of the pan. A steady rate of heat transfer from the stove to boil water in the pan is given by Q=k A (T1-T2) /L (Incropera, Dewitt, Bergman and Lavine, 2007, 126) Where, Q=Heat transferred into the pan A=Surface area of heat transfer T1=Temperature of the outer surface of the pan T2=Temperature of the inner surface of the pan L=Thickness of the pan a) If the pan is made of aluminium A=∏D2/4=3.142*0.22/4=0.03142m2 L=7.5mm=0.0075m kal=240 M/(m.K) The formula above, T1-T2=QL/(kA) T1=T2+ QL/(kA) Therefore, T1=T2+ QL/(kA)=150+645*0.0075/(240*0.03142)=150.64oC T2=150.64oC b) If the pan is made of copper All the values remain the same as in part (a) except for the k value, which vary with the material. kCu=390W/m.K T1=T2+ QL/(kA)= 150+645*0.0075/(390*0.03142)=150.39oC T1=150.39oC Figure 1: Pan set up Bibliography Incropera, F.P., Dewitt, D.P., Bergman, T.L., and Lavine, A.S., 2007. Fundamental of heat and mass transfer. 6th ed. Hoboken, NJ: John Wiley & Sons, Inc. New Hampton, 2008. 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