Given the enthalpy of formation data in the table below, what is the enthalpy of reaction for the reaction you performed in this lab? How does this compare to your experimental results? To calculate the enthalpy of reaction, use the formula below. AHran=EAH; (products) - EAH; (reactants Note that you will need the balanced chemical equation for the reaction performed in the lab, which can be found in the Background in your Hayden-McNeil course site. Also note that AH₁° for standard state elements is 0 kJ/mol.

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In some parts of the world, butadiene was produced from ethanol, C2H&O by the unbalanced reaction: C2H60 (g) → C4H6 (g) + H20 (g) + H2 (g) 1. Balance the above reaction. I'd like you to determine whether this reaction is exo- or endothermic, but you need more information first. The following questions will walk you through this process. 2. Given the reaction and thermochemical data below, use Hess' Law to calculate A H,xn for the gas-phase combustion of butadiene. 11 O2 (g) = ? kJ C4H6 (g) + 4 CO2 (g) + 3 H20(1) - 2 H2O(g) A H; = -484 kJ 2 H2 (g) + O2 (g) + 6 02 (9) 4 CO2 (g) + 4 H2O(g) AHxn =-2527 kJ C4H8 (g) AHxn =+132 kJ C4H8 (g) C4H6 (g) + H2 (g) AHvap = +41 kJ H20 (1) H2O (g)

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A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Ignition wires heat sample Water Stirrer Thermometer Insulated Sample Burning Steel outside dish sample bomb chamber Combustion (bomb) calorimeter. In an experiment, a 0.4370 g sample of benzoic acid (CH6O₂) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.043 x 10³ g of water. During the combustion the temperature increases from 22.78 to 25.08 °C. The heat capacity of water is 4.184 J-g¹. C¹. The heat capacity of the calorimeter was determined in a previous experiment to be 893.1 J. "C Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of benzoic acid based on these data. CHO₂(8)+(15/2)O₂(g) → 3H₂O(l) +7C0₂ (9) + Energy Molar Heat of Combustion= kJ/mol

In this problem you are going to determine the molarity of a strong acid solution by measuring the enthalpy change of the acid’s reaction with a base, which causes the temperature of the reaction mixture to go from 22.3 °C to 34.8 °C. You will have to look up values from your OpenStax text. A)  What is the underlying reaction of every acid-base neutralization reaction? What is the enthalpy change of this reaction per mole of acid? B) You performed this acid-base neutralization reaction with 100.0 mL of 2.00 M sodium hydroxide (base) and 60.0 mL of your unknown strong acid. What is the total volume of your reaction mixture after you mix the two solutions together? (The base is in excess.)

7. Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis structure for each molecule. CH, (g) + 20, (g) ·CO, (g) + H,O (g) Bond Bond Enthalpy (kJ/mol) C-O 351 C=0 799 CEO 1070 O-O 142 O=0 498 C-H 414 O-H 460

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Question 36

Questions Suppose the calorimeter used for this experiment had been made of a heat-conducting material (such as metal) rather than plastic foam, so that the portion of heat energy lost to the calorimeter itself was larger and could not be ignored. Would the temperature changes experienced when mixing the acid with the base have been larger or smaller? Justify your answer. 1.