The heat of combustion of acetylene, F2H2(g) + O2(g) → CO2(g) + H20(g) A „H° = -1300 kJ mol*1 %3D (a) Calculate the heat generated (in kJ) by burning 2.747 g of acetylene. We are looking for the absolute value of the heat here. = 137.1 V o kJ (b) If all the heat is transferred to a 2.292 kg sample of water, originally at 24.788 °C calculate the final water temperature. °C. (Enter the correct number of significant figures) Enter an integer or decimal number, with exactly 5 significant figures [more..]

The heat of combustion of acetylene, F2H2(g) + O2(g) → CO2(g) + H20(g) A „H° = -1300 kJ mol*1 %3D (a) Calculate the heat generated (in kJ) by burning 2.747 g of acetylene. We are looking for the absolute value of the heat here. = 137.1 V o kJ (b) If all the heat is transferred to a 2.292 kg sample of water, originally at 24.788 °C calculate the final water temperature. °C. (Enter the correct number of significant figures) Enter an integer or decimal number, with exactly 5 significant figures [more..]

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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Hydrogen peroxide, H2 O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2 O2 can be prepared in a process whose overall change is H2 (g) + O2 (g) –→ H2O2 (1) Calculate the enthalpy change using the following data: 2H2О2(1) — 2H,0() + О-(9); дн: -196.0 kJ На (9) + 3 О2(9) > H20(1); дН — — 285.8 kJ = - ΔΗ - kJ
Consider the following thermochemical equation: 2X2Y6(g) + 7O2(g) ⟶ 4XO2 + 6Y2O Δ?= -2.615 x 103 kJ Calculate the enthalpy change when 16.38 g of XO2 are produced in this reaction. The molar mass of XO2 = 47.28 ???? Report your answer as a positive number, in kJ, with 4 significant figures.
What is the change in the enthalpy (in kJ) for the complete combustion of 39.0 g of fructose, roughly the amount of sugar in a 12-oz can of soda? C,H12O6 (s) + 602(g) → 6CO2(g)+6H,O(1) AH = -2.83 × 10° kJ mol¬1 A: -6.13 x 102 3703
In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Ammonia burns in the presence of a platinum catalyst to produce nitric oxide, NO: 4 NH, (g) + 5 0, (8) → 4 NO(g) + 6 H, O(g) What is the heat of reactiorfin kJ mol1 for the reaction above using the following data? Reaction AH (kJ mol¯') 180.6 N2(g) + O2(g) → 2 NO(g) N2(g) + 3 H2(g) → 2 NH3(g) -91.8 2 H2(g) + O2(g) → 2 H20(g) -483.7 Enter your value in the first box and an appropriate unit of measure in the second box.
Styrene (C8H8) is one of the substances used in the production of synthetic rubber and burns according to the following combustion reaction C8H8(l)+10O2(g)-->8CO2(g)+4H2O(l). Hrxn=-4.390x10^3 jk/mol what is the standard enthalpy of formation at 25 degrees Celsius? Hf[CO2(g)]=-393.5 kj/mol Hf[H2O(l)]=-285.8 kj/mol
When ammonia reacts with dinitrogen oxide gas (ΔHf° = 82.05 kJ/mol), liquid water and nitrogen gas are formed. How much heat is liberated or absorbed by the reaction that produces 365 mL of nitrogen gas at 25°C and 743 mm Hg? (in kJ) ΔHf° (kJ/mol) NH3(g) –46.1 H2O(l) –285.8 N2(g) 0 N2O(g) 82.05
For the questions of the Experiment of Heat and Temperature: The Law of Dulong and Petit, the following data were obtained for the unknown element. specific heat (S) of unknown element (J/g⚫K) Aw of unknown element (g/mol) 0.339 63.96 b) Calculate the atomic heat (C) in J/mol K for the unknown element. 1) In this case, your answer should be in decimal notation (for example, 0.123, not 1.23*10^-1) with the correct number of significant figures. Also follow the unit specified in each question. Do NOT put its unit in your answer because its unit is shown already in the questions. 2) It means students shouldn't include any letters or text in the "Numeric answers", because otherwise it'll be marked wrong even if the numbers are correct. Type your answer...
For reaction (b) HCl(g) + NaOH(s) NaCl(s) + H20(I), what is the equation for the change in enthalpy of this reaction? O [AHf° (NaCI(s)) + AHf°(H20(1)] - [AHP(HCI(g)) + AHP(N2OH(s))] O [AHP (HCI(g)) + AHP(N2OH(s))] - [AHP(NaCI(s)) + AHP(H20(1))] Click if you would like to Show Work for this question: Open Show Work SHOW HINT SHOW SOLUTION Part 4 X Your answer is incorrect. Try again. Use the values from the given table and the equation you chose in Part 3 to find the overall change in enthalpy for the reaction. -55200
Calcium oxide (CaO) is used to remove sulfur dioxide generated by coal-burning power stations: 2CaOs + 2502i) + O21) → 2CaSO4s) What is the heat (in kJ) involved for this removal process if 6.6 g of SO2 (64.07 g/mol) is converted? AH (Cao) = -635.6 kJ/mol AH; (SO2) = -296.1 kJ/mol AH?(CasOa) = -1432.7 kJ/mol
When exactly one mole of chrysene, C18H12(s) is burned at 25°C in a calorimeter, ΔE = -8942.6 kJ. When any hydrocarbon like chrysene is burned completely, the products are CO2 and H2O. (a) Write and balance the chemical equation for the combustion reaction of chrysene. (Use the lowest possible coefficients. Include states-of-matter under the given conditions in your answer.)(b) Determine the value of ΔH per mole for the combustion of chrysene at 298 K (25°C). kJ/mol(c) When 1.1112 g of chrysene C18H12(s), was burned in a bomb, the temperature rose from 21.82°C to 25.28°C. What is the heat capacity of this calorimeter? kJ/°C
lgs everything else). e system (the part you are studyml (reaut nsi ost systems we are interested in will have a constant pressure, mean ing that q (heat or thermal energy) would be equivalent to the change in enthalpy (AH) We defined environments in which heat goes into the system surroundings get hot as exothermic ΔΗ- and the surroundings get cold as EX rmic AH + while environments in which heat goes out of the system and the For each of the environments below: (1) identify your system and surroundings and (2) predict whether it would be endothermic or exothermic. 1. a. Wood burning b. Water freezing c. Sweat evaporating d. Chemical hand-warmer
and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8