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    Multiple Choice

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    C60; ΔH = 2320 kJ what is ΔH for the following thermochemical equation? 1/60C(s)>>>> C(s) A) +38.7 kJ B) +2320 kJ C) -129 MJ D) -2320 kJ E) -38.7 kJ E is the correct answer. Since the forward reaction has a positive enthalpy‚ the reverse will have a negative enthalpy. Also we are dealing with 1/60th of the original amount‚ so (2320 kJ)*(1/60 mol)*(-1) = -38.7 kJ 3. Exactly 173.9 J will raise the temperature of 10.0 g of a metal from 25.0°C to 60.0°C. What is the specific heat capacity

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    Specific Heat Lab Report

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    Specific Heat Lab Report “Here are the facts we confront; No one is against conservation. No one is against alternative fuel sources.” – J. D. Hayworth Research Question: Does the number of hydrocarbons that a fuel is composed of affect how much it will ignite? If so‚ consider the following: What is the quantity and concentration of the combustion that is released and how can that be measured in other (more coherent) means? These are the fuels that were seasoned throughout the

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    Combustion Of Alcohols

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    Reaction co-ordinate ?H is the heat content‚ which is the enthalpy‚ which is negative in exothermic reactions as the diagram shows that energy is ’lost’ as heat. Enthalpy is defined as the energy of reaction‚ or the heat energy associated with a chemical change. Chemical Principles By Master & Slowinski says that "For any reaction carried out directly at a constant pressure‚ the heat flow is exactly equal to the difference between enthalpy of products and that of the reactants"‚ or: Qp = Hp - Hr =

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    I need help

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    Zn(s) + CuSO4(aq) ------ Cu(s) + ZnSO4 (aq) The enthalpy changees for two different reactions will be determined practically. In the first‚ experiment delta H will be determined directly and account will be taken of heat losses by extrapolation of an appropriate graph. The second experiment involves teh inderect determination of an enthalpy change using Hess’ Law. The temperature can be measured manually but this experiment is ideal for using a data logger. In the first experiment we are trying

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    Bomb Calorimetry

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    The goal of this experiment is to determine the enthalpy of combustion of naphthalene by means of a bomb calorimeter. First‚ the bomb calorimeter was standardized using benzoic acid and the average heat capacity of the bomb calorimeter was calculated to be 10.60.3205 kJ/K. From that‚ the These results show that heats of combustions of unknown substances can be determined via bomb calorimetry. Introduction The first law of thermodynamics states that energy is conserved.2 Using that law it can

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    Calorimetry Intro

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    Greek metry meaning to measure‚ is the science of measuring the amount of heat‚ q.1 The amount of heat is absorbed (endothermic where qrxn >0) or released (exothermic where qrxn <0) by the system with respect to its surroundings is the change in enthalpy‚ ΔH. This is quantified in calorimetry by a device called calorimeter. There are two types of calorimeters. The first type is the called the bomb calorimeter. It is ideally suited for measuring the heat evolved in a combustion reaction. Because

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    IB Math Exploration

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    Determining the Enthalpy of Combustion of a Wood Chip IB Chemistry 12 September 18‚ 2014 Ryan Ingham Table 1: Raw data collected from the temperature probe and scale for the water‚ the aluminum can and the wood chip. (Quantitative) Quantity Initial Temperature (±0.1K) Final Temperature (±0.1K) Aluminum Can 46.29g (±0.01g) 296.5 314.7 Water 250g (±0.1g) 296.5 314.7 Wood Chip Before: 4.64g(±0.01g) After: 3.29g (±0.01g) NA

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    Chem122 Midterm 1

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    NO books‚ lecture notes‚ cell-phones‚ PDAs‚ laptops‚ talking. For Multiple Choice Problems (on the back) - Circle your answer to each question BELOW. If more than one answer is circled for a question no credit will be given for it. 1. [ out of 16 pts ] A mixture of gases contains 66.0 g CO2‚ 2.02 g of H2‚ and 16.0 g of O2. If the total pressure of the mixture is 725 torr‚ what is the partial pressure of each gas? [ do not neglect significant figures! ] SHOW YOUR WORK to

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    Heat of Neutralization

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    measured the temperature of the system for the next three minutes. I could then use the data collected to determine the heat of neutralization for the reaction. The scientific principles addressed by the lab were using a calorimeter to measure the enthalpy change (or heat of reaction) of a system‚ and determining how much heat was

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    to solve for the specific heat of the metal. The molar mass of the metal was found by using the equation: MM = 25 / C (J/g° C) Experiment B was conducted to find the heat of solution of an unknown solid. After finding the heat flow of the water‚ enthalpy change of the reaction was found by using the equation: Q reaction =  H

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