2 attempts leftCheck my workEnter your answer in the provided box.Acetylene burns in air according to the following equation:5C₂H2(g) + + O2(g) →2 CO2(g) + H2O(g)00ΔΗ=-1255.8 kJrxnGiven AH of CO2(g)=-393.5 kJ/mol and AH of H2O(g)=-241.8 kJ/mol, find AH of C2H2(g).0fkJ/molHintSolutioGuided Sol

To find the standard enthalpy of formation (ΔHf∘) of acetylene (C2H2), we can use the given…

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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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34510/variants/434510/take/10/ Question 11 Draw a complete enthalpy diagram for the following reaction: 4Na) + O2(g) → 2Na₂O(s) PO AH = 178 kJ PENCIL THIN BLACK a + 07 12
Using standard heats of formation, calculate the standard enthalpy change for the following reaction. 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) AH (NH3 (9))=-46.1 kJ/mol AH (N₂O(g)) 82.1 kJ/mol AH (N₂(9))= 0.0 kJ/mol AH (H₂O(g))=-241.8 kJ/mol AH rxn kj
5) Mothballs are composed primarily of the hydrocarbon naphthalene (C₁0H8). When 1.025 g of naphthalene burns in a bomb calorimeter, the temperature rises from 24.25 °C to 32.33 °C. What is the heat for the combustion of naphthalene in kJ/mol? The heat capacity if the bomb calorimeter was determined to be 5.11 kJ/°C.
1. What is 4-H for this reaction: 3C(s) + 4H2(g) → C3H8(g) given the following reactions: C3H8(g) +502(g) → 3CO2(g) + 4H2O(g) C(s) + O2(g) → CO2(g) 4-H = -2043 kJ/mol AH = -393.5 kJ/mol 4,H= -483.6 kJ/mol 2H₂(g) + O2(g) → 2H₂O(g) (a) -4191 kJ/mol (b) 1166 kJ/mol (c) 378 kJ/mol (d) -105 kJ/mol
Consider the following thermochemical equations (Note: HA is a weak acid)H+(aq) + OH-(aq) → H2O(l) ΔH1HA(aq) → H+(aq) + A-(aq) ΔH2HA(aq) + OH-(aq) → A-(aq) + H2O(l) ΔH3Choose the equation that shows the correct relationship between their enthalpy changes.
Calculate the heat released (kJ) in the reaction of 3.50 g of acetylene (C2H2) and excess hydrogen gas to form ethane gas: C2H2(g) + 2H2(g) → C2H6(g) Given: 2C2H2(g) + 502(g) → 4CO2(g) + 2H20(g) AH = -2320 kJ/mol 2C2H6(g) + 702(g)→4CO2(g) + 6H20(g) AH = -3040 kJ/mol 2H2(g) + O2(g) 2H20(g) AH = -572 kJ/mol Multiple Choice None of the above 30.5 kJ 29.5 kJ 28.5 kJ 27.5 kJ
Ignition wires heat sample Thermometer Stirrer 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. In an experiment, a 0.4059 g sample of 9,10-anthracenedione (C14H30,) is burned completely in a bomb calorimeter. The calorimeter is surounded by 1.116x10³ g of water. During the combustion the temperature increases from 22.76 to 25.09 °C. The heat capacity of water is 4.184 Jgl°c-!. Water The heat capacity of the calorimeter was determined in a previous experiment to be 965.5 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of 9,10-anthracenedione based on these data. C14HgO2(s) - 1502(g) 4 H20(1) + 14 CO,(g) - Energy Molar Heat of Combustion = kJ/mol Sample dish Burning sample Steel Insulated outside chamber bomb Combustion (bomb) calorimeter.
18. From the following data, AH = -393.5 kJ/mol C(graphite) + O₂(g) → CO₂(g) 1 H₂ (g) + O₂(g) → H₂O(l) AH = -285.8 kJ/mol 2C₂H6 (g) +70₂(g) → 6H₂O(l) + 4CO₂(g) AH = -3119.06 kJ/mol calculate the enthalpy change for the reaction: 2C (graphite) (1) + 3H₂(g) → 2C₂H6 (g)
Calculate AH for the following reaction, given the data in the table below: H2SO4() → So:(g) + H2O(g) AH = ??? kJ/mol H2S(g) +202(g)→ H2SO4(1) AH = -749.7 kJ H,S(g) + 202(g) → SO3(g) + H2O(1) AH = -355.0 kJ H20(1) H20(g) AH = +53.95 kJ
Please help me, double and triple check your answers previous tutors got it wrong,
Calorimetry: Question #3 Octane, C3H18 , is a constituent of gasoline, and burns in the presence of oxygen to produce water and carbon dioxide: 2 C3H18 (1) + 25 O2(g) → 16 CO2(9) + 18 H2O1) ΔΗ kJ/2mol %3D rxn C3H18 (1) When a 1.00-gram sample of octane is burned in a bomb calorimeter the temperature of the water and the calorimeter rises from 25.00°C to 33.20°C. If the heat capacity, Cbomb cal, of the empty bomb calorimeter is 837 J/°C, and the mass of the water is 1.200 kg: a) Calculate the heat, q, transferred, during the combustion, to the calorimeter: 6.86 kJ (calorimter) + qbomb cal = Cbomb cal • AT b) Calculate the heat, q, transferred, during the combustion, to the water: 41.2 kJ (1.200 kg H20) + 9H20 = + mH20 • AT • SH2O c) Calculate the enthalpy change (AHº rxn = kJ/2mol) for this reaction (2 mol of C3H18 (1): [ Select ] kJ/2 mol C3H18 (1)
Given the enthalpies for the following reactions: 2 Fe (s) + 3/2 O₂(g) → Fe2O3 (s)Math output error AH₂ ΔΗ, CO (g) + 1/2 O₂ (g) → CO₂ (g) CO2 (g) ΔΗ = -248.7 kJ rxn rxn = 1,091.6 kJ Calculate the enthalpy change (AHrxn) for the following reaction: Fe2O3 (s) + 3 CO (g) → 2 Fe (s) + 3 CO₂ (g)

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