Introduction A fuel is burnt and as much of the energy released as possible is transferred to water by heating. Using the fact that 4.18 J of energy are required to raise 1 g of water by 1 °C, the amount of energy given out by the fuel can be calculated. This can then be converted to the amount of energy given out per mole in order to calculate the enthalpy change of combustion of the fuel. Pre-lab questions 1 The water is contained in a metal can. Why is a metal can used and not a glass beaker or other similar container? Ethanol and propanol were chosen for this experiment as they are members of a homologous series. Identify the homologous series to which they belong and give the next member of the series. One of the biggest causes of error in this experiment is heat loss. Does this lead to systematic or random errors? Suggest how these errors could be decreased.

Introduction A fuel is burnt and as much of the energy released as possible is transferred to water by heating. Using the fact that 4.18 J of energy are required to raise 1 g of water by 1 °C, the amount of energy given out by the fuel can be calculated. This can then be converted to the amount of energy given out per mole in order to calculate the enthalpy change of combustion of the fuel. Pre-lab questions 1 The water is contained in a metal can. Why is a metal can used and not a glass beaker or other similar container? Ethanol and propanol were chosen for this experiment as they are members of a homologous series. Identify the homologous series to which they belong and give the next member of the series. One of the biggest causes of error in this experiment is heat loss. Does this lead to systematic or random errors? Suggest how these errors could be decreased.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Use the following information to answer Questions 6-9: A sample of NH4NO3 with a mass of 5.0 g is dissolved in 40.1 g of deoinized water in a calorimeter. The initial temperature of the water is 21.2 oC. The final temperature of the solution is 15.4 oC. The calorimeter constant = 25.2 J/oC. If qH2O = -910 J and qcal = -130 J for 5.0 g of NH4NO3, calculate the heat of solution in J per gram of NH4NO3.
5. In question 1, you calculated the enthalpy change for the combustion of propane from combining 3 reactions with known enthalpy changes using Hess's Law. Alternatively, standard heats of formation are a general method to find the enthalpy change in ANY reaction from information that can be looked up in a table. C₂H₂(g) -103.85 CO₂(g) -393.5 H₂O (1) H₂O(g) a) -285.8 -241.8 Use the tabulated heats of formation and the equation connecting standard enthalpy change of reaction to standard enthalpy change of formation of reactants and products to calculate AH for the combustion of propane in kJ/mol. Compare this with your answer to 1. b) Why did you not need a tabulated value of AH', for O₂ (g)?
Reactions are classified as either exothermic or endothermic. Exothermic reactions feel hot (e.g., a burning campfire), whereas endothermic reactions feel cool (e.g. squeezing an instant cold pack). A thermometer measures the temperature of the surroundings in a calorimeter to determine the amount of energy being transferred by the system. Water molecules speed up when they gain heat and slow down when they lose heat; note that you can track both the cold and hot water molecules in the simulation based on the shade of red of the larger central oxygen atom by checking the box labeled Show microscopic view. Select the Experiment tab in the simulation, and then click Run Demonstration. When observing the simulation, pay particular attention to the temperature change and movement of the molecules by clicking Show microscopic view when HCl and NaOH neutralize each other in the fourth experiment. Use your observations to complete the following sentences. Match the words in the left column to…
When 0.361 g of sodium metal is added to an excess of hydrochloric acid, 3750 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) + 2 HCI(aq) 2 NaCl(aq) + H, (g) Enthalpy of reaction: kJ about us careers privacy policy terms of use contact us help 10:51 PM (? 10/15/2020
Pre-laboratory Assignment: Calorimetry and Hess’s Law
Answer all the questions and show your solution.
Please dear not hand written please.
please answer D.
According to question 3 from The Additivity of Heats (Hess's Law) Worksheet what is the change in enthalpy (kJ) for the following reaction? Do not type units into your answer. SiO2(s) + 4HF(g) ⟶ SiF4(g) + 2H2O(l) Δ?=?
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ORT SHEET Heat of Neutralization EXPERIMENT elemsboomfchg lom 12 A. Heat Capacity of Calorimeter 1. Temp. of calorimeter and water before mixing 2. Temp. of warm water °C 22.0 39,0 30.3 3. Maximum temp. determined from your curve °C 4. Heat lost by warm water (temp decrease x °C 50.0 g x 4.184 J/K-g) = 02), 5. Heat gained by cooler water (temp. increase x 50.0 g x 4.184 J/K-g) = 30,3 22.0)x 13626J s0.0gmpi S0.0gy 6. Heat gained by the calorimeter [(4) – (5)] = 7. Heat capacity of calorimeter: heat gained by the calorimeter temperature increase J/K 3. Heat of Neutralization of HCl-NaOH 22.2 22.2. °C . Temp. of calorimeter and NaOH Temp. of HCI AT determined from your curve after adding HC1 °C to the NaOH Heat gained by solution (temperature increase x ON 100 g x 4.184 J/K-g) = 9977.8J %3D Heat gained by calorimeter (temperature increase x heat capacity of calorimeter) = J %3D Total joules released by reaction [(3) + (4)] = Tight O 2018 Pearson Education, Inc.