Bomb Calorimeter Lab Report

Weight 10 dry post-82 pennies which get 77.12g, using 30ml initial volume measuring the volume of 10 pennies, record the data 9.1ml. Using equation Density= Mass/Volume, get the density of the pre-82 pennies is 8.47g/ml. Then calculate the error%=0.04%, and the deviation%=7.13%.

The percentage error for both trials came to 79.6% and 85% so if only 20% of the energy was released onto the can the rest of it was released into the atmosphere and its surrounding areas. As a result, the amount of energy being released onto the can was short but the rest of energy eventually released at a high percentage because the energy does not disappear, but the energy goes out to surrounding and the air. Significantly, every calculation was taken accurately but the error percentage somehow proved inaccurate because we used the equation Q=m*Cp*T to calculate how much energy was being released by the sample and then we also used it calculate the Calories per gram which there we figured out the changes within the experiment then when we subtracted the result and divided it by 6.4 then times it by 100 it gives the amount of the percentage error to determine how much energy was released and find out where it ended all up to be. In conclusion, the energy released during combustion reaction goes to the air and everything else around the energy because due to the amount energy being released it can tell us how much energy went missing and find out where it all went to determine the error that went on during the

Because it is dangerous to burn magnesium, it is not possible to directly record heat change. Our lab team suggests an indirect way of determining the heat of combustion for magnesium. To accomplish this, we need to perform two separate trials. One uses a solid (powder) version of MgO, while the other uses Mg ribbon. With the results from these, we can use Hess’ Law to determine q=∆H. This provides both a safe and successful way of indirectly determining the heat of combustion for magnesium.

A more detailed explanation of procedures can be found in the lab packet.1 To summarize, samples of benzoic acid and naphthalene were combusted using the Parr 1341 Calorimeter with a Parr oxygen bomb. A massed benzoic acid pellet was placed onto the center of the combustion pan and 10 cm of nickel alloy fuse wire was massed and then threaded through both electrodes on the head of the bomb so that it lay firmly against the acid pellet. 1mL of distilled water was then placed in the bottom of the bomb in order to ensure that all the water produced by the

People never want to acknowledge the fact that many prisoners who are imprisoned went through tough hardships in life yet, they have real talents that can surprise the nation. In this essay I will discuss three articles that talk about racism towards blacks by splitting them into four groups, life about prisoners who are missing from everyday life and the hardships of a prisoner Theothus Carter. Eugene Robinson’s “Disintegration” will discuss how the disintegration that many people has caused amongst the blacks and splitting these blacks into four groups and separated by demography, geography, and psychology. With that, They have different profiles, different mindsets, different hopes, fears, and dreams. In addition, Justin Wolfers article

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

Calorimetry is the analysis of energy changes in a certain system by determining how heat interacts within the system and with its surroundings. Bomb calorimetry, also known as constant volume calorimetry, is a method used in determining the enthalpy of combustion of a given hydrocarbon through the analysis of heat exchange in chemical reactions. The enthalpy of the substance is determined by many factors, including the heat capacity of the calorimeter, moles of substance lost during combustion, and the number of gas molecules lost post-combustion, to name a few. The relationship among the given factors were studied and applied in determining the enthalpy of combustion of a naphthalene (C10H8) sample. A standard bomb calorimeter, together with

When the fuels are burnt, energy is given off. I will be calculating the energy given off using the formula above. The specific heat capacity is the energy

Reaction kinetics in the Monopropellant Flame is also captured in a simple Arrhenius expression (Equation 3.4) to determine mass flux. m_AP= A_AP exp(-E_AP/RT_AP ) (3.4) In the Monopropellant Flame the reaction rates are fast and are not impeded by diffusion since the gaseous AP decomposition products are reactive components that are already in close proximity. The flame standoff distance of the Monopropellant Flame is governed largely by pressure and is calculated using Equation 3.5 and then expressed as a dimensionless parameter in Equation 3.6.

In order to measure the heats of reactions, add the reactants into the calorimeter and measure the difference between the initial and final temperature. The temperature difference helps us calculate the heat released or absorbed by the reaction. The equation for calorimetry is q=mc(ΔT). ΔT is the temperature change, m is the mass, c is the specific heat capacity of the solution, and q is the heat transfer. Given that the experiment is operated under constant pressure in the lab, the temperature change is due to the enthalpy of the reaction, therefore the heat of the reaction can be calculated.

    In this lab, a calorimeter was used to find the enthalpy of reaction for two reactions, the first was between magnesium and 1 molar hydrochloric acid, and the second was between magnesium oxide and 1 molar hydrochloric acid. After the enthalpy for both of these were found, Hess’ law was used to find the molar enthalpy of combustion of magnesium, using the enthalpies for the two previous reactions and the enthalpy of formation for water. The enthalpy of reaction for the magnesium + hydrochloric acid reaction was found to be -812.76 kJ. The enthalpy of reaction for the magnesium oxide + hydrochloric acid reaction was found to be -111.06 kJ. These two enthalpies and the enthalpy of formation for water were manipulated and added together using Hess’s law to get the molar enthalpy of combustion of magnesium. It was found that the molar enthalpy of combustion of magnesium was -987.5 kJ/mol. The accepted enthalpy was -601.6 kJ/mol, which means that there is a percent difference of 64%. This percent difference is very high which indicates that this type of experiment is very inefficient for finding the molar enthalpy of combustion of magnesium. Most likely, a there are many errors in this simple calorimeter experiment that make it inefficient for finding the molar enthalpy of combustion of magnesium.

If 10.0g of solid baking soda is poured into 30 mL of citric acid, then a reaction will occur and an increase in temperature will be observed. Whereas, if a piece of magnesium metal is added to 30 mL of Hydrochloric Acid, then a reaction will occur and an increase in temperature will be observable. For Part 3 of the experiment, if 50 mL of tap water is placed in a can 2.5 cm inches above a burning marshmallow, then through the process of calorimetry the energy content of the marshmallow should be 5.0kJ/g (the value provided by the United States Department of Agriculture).

Purpose: To utilize a calorimeter correctly to find the enthalpy changes in two different reactions. The purpose was also to use concepts of specific heat to observe the relationship between temperature observations and heat transfer. Then, use the equations to see the relationship between change in energy and the amount of substance involved. Use Hess’ law to determine the change in energy.

In this investigation I will be burning alcohol 's to heat up a can of water. I will be burning four alcohol 's, methanol, ethanol, propanol and butanol. The aim is to find out how much energy is produced when burning these alcohols. Alcohol 's react with oxygen in the air to form water and carbon dioxide.

We think the tests we did went smoothly and we had no problems, except for the fact that we broke one of the test tubes from school. After all it was under a flames for majority of the experiment, the thermometer slipped 1 cm from the bottom of the test tube and shattered a hole through the bottom of it. Threw our experiment we had to keep our variables the same by even having the test tube with water at the exact same height every time above the burning flame . We also kept the same amount of gel fluid the same in every test that is why it was surprising to us that the gel by itself would heat the tube with water in it to higher temperature. We think this is because the gel added with the caramelized fizzy drink had to use a lot more energy to start the reaction which was boiling the excess fizzy drink to create a warm flame that could not last as long because it was using the gel to create energy.