Monopropellant Flame Lab Report

Combustion Reaction: A chemical reaction between a fuel and an oxidizing agent that produces heat.

For the test tube with the ratio of Acetylene to air is 1:3, a flame traveled down a test tube even slower, there was a slight popping noise and black residue . For the test tube with the ratio of Acetylene to air is 1:7, a flame traveled quickly down a test tube, popping noise and less black residue. Refer to table 1 for the specific lab results.

Please refer to Experiment 5 on page 79-84 of Laboratory Manual for Principles of General Chemistry by J.A. Beran. The only deviation that was observed in the experiment was due to a procedural change instructed by the professor to increase the flame were no observable deviations in the experiment.

The principle behind the extinguisher is simple: as they are mechanical pressure waves that cause vibrations in the medium in which they travel.

An Investigation into the Enthalpies of the Combustion of Alcohols = == == == ==

In a combustion reaction, a compound or element reacts with oxygen, releasing a large amount of energy in the form of light and heat.

CHE341Homework Assignment #10Due:Monday16Novemberat6:00PM1.Aunimoleculargas-phasereactionX→Yis activated with collisions by an unreactivecollision partner Bwith the following mechanism:X+Bk1k−1⎯→⎯⎯←⎯⎯⎯X*+B,X*k2⎯→⎯Y,has a rate that follows the effective rate equationdY[]dt=kuniX[]. (a) Apply the steady state approximation (SSA) to determine an algebraicexpression forkuniin terms terms of the rate constantsk1,k–1andk2as well as [B]. (b)Discusshow the rate law changes in the limit of large and small [B].2.Dissociation of ethane into methyl radicalsfollowsfirst-order kinetics with ArrheniusparametersA=2.50×1016s–1andEa=367.6kJ mol–1. Calculate the Gibbs energy ofactivation, the entropy of activation and the enthalpy of activation at500 K.3.

The weight of the fuel and the rate of spread affect fire intensity by increasing or decreasing it, which in turn affects the fireline intensity. The heavier the fuel is, the more there is and the faster the spread therefore increasing both the fire intensity and fireline intensity. The lighter the fuel, the less there is and the slower the spread therefore decreasing both types of intensities. Heat per Unit Area (HA) is the total heat released from a given area (kJ m-2).

Having a basic torch, there will be two valves by the handle. On different torches there are different ways to control how much acetylene and oxygen are coming out of it. On the basic torch, one valve controls your amount of acetylene, and the other controls the amount of oxygen. Both are concentrated out of the tip of the torch. The acetylene valve is connected to

If the volume of the combustion container is 10.0 L, calculate the final pressure in the container when the temperature is changed to 110.° C. (Assume no oxygen remains unreacted and that all products are gaseous.)

Once the change in temperature is determined, the Cv equation for benzoic acid can be utilized. C_(v,cal)=((∆cH_b-∆nRT/m_b ) m_b+C_Fe+C_N)/∆T (3) Where ∆cHb is the benzoic acid heat of combustion, CFe is the iron fuse wire correction for combustion, T is the initial temperature, ∆n is the change in moles of the gas in combustion, and Cn is the nitric acid formation correction factor. After the calibration of the bomb calorimeter, the heat of combustion of the sucrose and altoid mint were calculated using the following

The heat absorbed or released from a system under constant pressure is known as enthalpy.(Khan Academy)This is because as the number of Carbon atoms increase. The chain of hydrocarbons will also be added to thus making it longer. As we move down the homologous group, the chain grows longer in size this is due to the additional CH3 Molecules added onto every next Alcohol within the group. Thus resulting in more energy being required to break apart the longer newly formed molecule. When reactions between any alcohol and an oxygen in the air they create C02 and H2O.(University of Texas)

As for the part two the experiment, the class was divided into two groups and both groups were specifically assigned to determine ΔS and ΔH. In order to determine ΔS and ΔH, the calorimeter apparatus was set up first. After, the materials that were also needed was the igniter and the fuel. The lab coordinator provided the groups with those materials. The igniter was initially weighted and was determined to be 0.057g. After, the initial weight of the igniter was recorded, it was then inserted to bottom of the fuel. Then the combination of the igniter and the fuel before the combustion was weighed, which was 0.647g. The igniter

Introduction: The theory behind this experiment is the heat of a reaction (∆E) plus the work (W) done by a reaction is equal to

The aim of this experiment was to test the heat of combustion over a period of time, and the energy required to combust alcohols with different carbon chain levels. It was hypothesised that the higher the carbon chain of the alcohol present, the faster the heat of combustion will occur. Meaning more energy will be released for a higher carbon chain. After calculating the results from the experiment it was found that the hypothesis was partially supported. The reasoning for this is as the alcohol that posses a higher carbon chain, generally increased there reaction rates. However there were a few exceptions to this rule.