Use and modify some/all the reactions provided to form the indicated overall reaction according to Hess' Law. • If a reaction is not used in your Hess' Law process, include that indication by multiplying the reaction by "0" • If no modification is needed and the reaction is applied as written below, include that indication by multiplying the reaction by "1" • Use whole numbers and simple fractions (such as "2" or "1/2", not 0.5) and negative signs (such as "-2") where needed Then calculate and report the enthalpy change (in kJ) for the overall reaction in the indicated blank, including units with your written value and rounded to 1 decimal place. Overall Reaction: CS2(1) + 302(g) → CO2(g) +2SO2(g) Rxn # Reaction ΔΗ° (kJ) 1 C(s) → C(g) 716.67 2 C(s) + O2(g) → CO2(g) -393.5 3 3Fe(s) +202(g) → Fe3O4(s) -1118 4 C(s) + 2S (s) → CS2(1) 87.9 5 CH4(g) + O2(g) → CO2(g) + H₂O(g) -882.0 S(s) + O2(g) → SO2(g) -296.8 N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(g) -629.1 6 7

Consider these reactions: Reaction 1: H₂(g) + Cl₂(g) 2HCl(g) AH = -184.6 kJ Reaction 2: 20F2(g) O₂(g) + 2 F₂ (g) ΔΗ = -49.4 kJ Reaction 3: N₂(g) +20₂ (8) 2NO₂(g) ΔΗ = +66.4 kJ

Consider the reaction.   2Fe2O3⟶4Fe+3O2      Δ?∘rxn=+824.2 kJ The formation of 77.0 g77.0 g of Fe results in -the absorption of 15900 kJ15900 kJ of heat. -the absorption of 1140 kJ1140 kJ of heat. -the absorption of 284 kJ284 kJ of heat. -the release of 284 kJ284 kJ of heat. -the release of 1140 kJ1140 kJ of heat. -the release of 15900 kJ15900 kJ of heat.

6. When 1 g of fuel Y is burned in a bomb calorimeter, the temperature of the calorimeter increases by 8.5 *C. The bomb has a heat capacity of 768 J/ "C and is submerged in 1200 ml of water. What is the heat of combustion of fuel Y in kJ/mole. Molar mass of fuel Y = 78 g/mole

EXPERIMENTAL DATA ΔΗ -55.84 kJ/mol neutralization Mass of dry calorimeter, (g) 126.73 Initial burette reading, (mL) 0.31 Final burette reading, (mL) 14.31 Initial temperature of HCI, (°C) 22.30 Initial temperature of NaOH, (°C) 22.34 Mass of calorimeter and NaCl solution, (g) 156.89 Extrapolated temperature, T;, (°C) 38.26

9:15 & a Part 1 Several chemical reactions happen in bioluminescent algae. One of the most important is cellular respiration, which along with photosynthesis helps produce the energy algae need to live. Cellular respiration can be represented by this chemical equation: 60₂ heat 6 CO₂ + 6H₂O + → C6H12O6 + glucose water oxygen carbon dioxide thermal energy 1. Since energy is released in cellular respiration, this reaction is exothermic. Why is the reaction exothermic, not endothermic? To answer this question, draw a model, create a graph, or write an explanation that includes: These materials were developed by the inquiryHub RPP, including educators from CO and IL, Northwestern University and the University of Colorado Boulder, with support from the Hewlett Foundation, the Spencer Foundation, the National Science Foundation and Denver Public Schools. Except where otherwise noted, this work is licensed under the Creative Commons Attribution 4.0 (сс O BY Hub International License. Version…

1. A student determines the molar mass of acetone, CH,COH., by the method used in this experiment. She found that the equilibrium temperature of a mixture of ice and water was 0.5°C on her thermometer. When she added 10.5 g if her sample to the mixture, the temperature, fell to -2.6°C. She then poured off the solution through a screen into a beaker. The mass of the solution was 86.4g. d. How much water was in the decanted solution?

* Ch. 5 Sect 4-5 ~ engine provides 572 Joules In this Push the Pistons. internal energy Chung by Calculate 9 for the represents carried by 1* An automobile of work Process to the -2683 Joules. Engine. This of heat be 300 the amount the cooling System

Enthalpy of Combustion (AH): 1. An alcohol is burned, and the heat is transferred to a large calorimeter that contains 3.0 kg of water. This combustion used up 0.285 moles of the alcohol and the temperature of the water to rose by 36.00°C. What is the enthalpy of combustion (AHC) of this alcohol in kJ/mol? (Remember that 1 kg = 1000 g) 2. When 1.20 g of hexane (C6H₁4) are burned, the temperature of 250.0 g of water is raised by 56.0°C. What is the enthalpy of combustion (AHC) of hexane in kJ/mol? 3. Use the following experimental data to determine the enthalpy of combustion of propanol (C3H₂OH) in kJ/mol Mass of water = 200.00 g Initial water temperature = 18.2°C Final water temperature = 38.6°C Initial mass of alcohol lamp = 185.51 g Final mass of alcohol lamp = 184.56 g subtract for massof stuff Know kJofq + mass of stuff 4. A 2.50 g sample of sucrose (C12H22011) was burned in excess oxygen in a bomb calorimeter that was surrou by 2,190 g of water. The temperature of the water…

Please help me , i need full solution. Please don't provide handwritten solution ..