2 C₂H6 (g)+7 02 (g) →4 CO2 (g) + 6 H₂O (e) ΔΗ° = − 3120 kJ When a sample of C₂H6 (g) is burned via the given equation, 396 kJ of heat is released. a) Calculate the mass of C₂H6 (g) burned. b) If the heat released by the reaction (396 kJ) is absorbed by 10.8 kg of bath water at 22.0 °C, what will be the final temperature of bath water? (Specific heat of water is 4.184 J / g °C). c) Considering the given reaction as system, state which of the following statements is correct if the reaction is carried out at constant temperature and pressure: work is done by the system on the surroundings; work is done by the surroundings on the system; no work is done. Explain your answer. (A detailed solution is required. Show all steps in the solution. Each quantity must be expressed with units and with correct number of significant figures.)

2 C₂H6 (g)+7 02 (g) →4 CO2 (g) + 6 H₂O (e) ΔΗ° = − 3120 kJ When a sample of C₂H6 (g) is burned via the given equation, 396 kJ of heat is released. a) Calculate the mass of C₂H6 (g) burned. b) If the heat released by the reaction (396 kJ) is absorbed by 10.8 kg of bath water at 22.0 °C, what will be the final temperature of bath water? (Specific heat of water is 4.184 J / g °C). c) Considering the given reaction as system, state which of the following statements is correct if the reaction is carried out at constant temperature and pressure: work is done by the system on the surroundings; work is done by the surroundings on the system; no work is done. Explain your answer. (A detailed solution is required. Show all steps in the solution. Each quantity must be expressed with units and with correct number of significant figures.)

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...

See similar textbooks

Similar questions

6. Calculate the amount of heat released when 1.26 x 104 grams of ammonia NH3 are produced according to the following equation. N₂ + 3H₂ → 2NH3 AH = -92.6 kJ
3
MISSED THIS? Watch IWE: Stoichiometry Involving AH; Read Section 7.6. You can click on the Review link to access the section in your eText. Titanium reacts with iodine to form titanium(III) iodide, emitting heat. 2Ti(s) +31₂(g) → 2Til3(s), AH = -839 kJ Part A Determine the mass of titanium that reacts if 2.30 x 10³ kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units. m(Ti) = Part B m(1₂) = μA Value Request Answer Ti Determine the mass of iodine that reacts if 2.30 x 10³ kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units. μA Value Units Request Answer ? Units ?
Please help me complete this question
The heat of reaction for the combustion of benzene (C6H6) is –3909.9 kJ. 2 C6H6 15 O2 → 12 CO2 + 6 H20 What would be the heat change when 161.54 g of benzene is burned in kilojoules?
Which of the reactions are exothermic? 2 Mg(s) + O,(g) → 2 MgO(s) + heat O NH, (g) + HCI(g) → NH,CI(s) + heat AgCl(s) + heat – Ag*(aq) + Cl¯(aq) 2 Fe, 0, (s) + 3 C(s) + heat → 4Fe(s) + 3 CO, (g) O C(graphite) + 0,(g) → CO,(g) + heat O CH, (g) + 20,(g) → CO,(g) + 2 H,O(1) + heat
Do not give handwriting solution.
A 5.43 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee cup calorimeter. Before placing the sample in the water, the temperature of the salt and water is 23.72°C. After the salt has completely dissolved, the temperature of the solution is 28.54°C. If -3.13 x 10 J of heat was lost during the dissolution reaction of 0.0465 moles of the unknown salt, what is the enthalpy change (in kJ/mol of salt) for the dissolution reaction? Type here to search
Consider the following equation for the combustion of H₂: 1 H₂(g) + H₂(g) + O₂(g) → O₂(g) → H H₂O(g) + 243 kJ In order to produce 972 kJ of heat, what mass of H₂ must burn?
2 moles of lithium metal reacts with liquid water to produce solid lithium hydroxide, hydrogen gas, and 402.4 kJ/mol of heat energy. a) write a balanced thermochemical equation for the reaction b) how much heat would be produced by the reaction of 14 g of lithium with an excess of liquid water c) is the reaction endothermic or exothermic?
How much heat is released during the combustion of 7.50 g of methane (molar mass = 16.0 g/mol)?
4. Determine the final temperature of water if 9.2 kJ of heat is added to 250 mL of 17°C water (the specific heat capacity of water is 4.184 J/g°C).