1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) +...
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1) C2H6 (g) -----> C2H4 (g) + H2 (g) ΔH1 = ? 2) C2H6 (g) + 3.5O2 (g) -----> 2CO2 (g) + 3H2O (l) ΔH2 = -1560 kJ/mo 3) C2H4 (g) + 3O2 (g) -----> 2CO2 (g) + 2H2O (l) ΔH3 = -1411 kJ/mol 4) 2H2O (l) -----> 2H2 (g) + O2 (g) ΔH4 = 571.6 kJ/mol How much heat is transferred between the system and the surroundings when 25 grams of ethane (C2H6) decomposes to produce ethylene (C2H4) and hydrogen gas? Is energy is released or absorbed by the system? *** Hint: You will need to calculate ΔH1 and use this value in your calculations to solve for this problem. ***
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Homework Answers
Given the thermo-chemical equations and their corresponding enthalpies of reaction: C2H6 (g) + 7/2 O2 (g)...
Given the thermo-chemical equations and their corresponding enthalpies of reaction: C2H6 (g) + 7/2 O2 (g) --> 2CO2 (g) + 3 H2O (l) ΔHRXN = -1560 kJ/mol 2C2H2 (g) + 5 O2 (g) --> 4 CO2 (g) + 2 H2O (l) ΔHRXN = -2599 kJ/mol H2 (g) + 1/2 O2 (g) --> H2O (l) ΔHRXN = -286 kJ/mol What is the standard enthalpy of reaction for the following? C2H2 (g) + 2 H2 (g) --> C2H6 (g)
Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ...
Given these reactions, where X represents a generic metal or metalloid 1) H2(g)+12O2(g)⟶H2O(g)Δ?1=−241.8 kJ1) H2(g)+12O2(g)⟶H2O(g)ΔH1=−241.8 kJ 2) X(s)+2Cl2(g)⟶XCl4(s)Δ?2=+157.3 kJ2) X(s)+2Cl2(g)⟶XCl4(s)ΔH2=+157.3 kJ 3) 12H2(g)+12Cl2(g)⟶HCl(g)Δ?3=−92.3 kJ3) 12H2(g)+12Cl2(g)⟶HCl(g)ΔH3=−92.3 kJ 4) X(s)+O2(g)⟶XO2(s)Δ?4=−769.5 kJ4) X(s)+O2(g)⟶XO2(s)ΔH4=−769.5 kJ 5) H2O(g)⟶H2O(l)Δ?5=−44.0 kJ5) H2O(g)⟶H2O(l)ΔH5=−44.0 kJ what is the enthalpy, Δ?,ΔH, for this reaction? XCl4(s)+2H2O(l)⟶XO2(s)+4HCl(g)
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data....
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
Compounds with carbon-carbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation...
Compounds with carbon-carbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation C,H (9) + H2(g) + C H (9) Calculate the enthalpy change for this reaction, using the following combustion data: C4H4 () + 30 (g) + 2CO3(g) + 2H2O(); AH = -1411 kJ C, H(g) + O2(g) → 2002(g) + 3H2O(l); AH = -1560. kJ H2(g) + O2(g) H2O(l); AH = -286 kJ Enthalpy change - KJ Submit Answer Try Another Version 10 item...
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−600.0 kJ HCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ...
Consider these reactions, where M represents a generic metal. 2M(s)+6HCl(aq)⟶2MCl3(aq)+3H2(g)ΔH1=−600.0 kJ HCl(g)⟶HCl(aq) ΔH2=−74.8 kJ H2(g)+Cl2(g)⟶2HCl(g) ΔH3=−1845.0 kJ MCl3(s)⟶MCl3(aq) ΔH4=−215.0 kJ Use the given information to determine the enthalpy of the reaction 2M(s)+3Cl2(g)⟶2MCl3(s) ΔH= kJ
Given the following reactions and subsequent delta H values, C2H6 (g) -> C2H2 (g) + 2H2...
Given the following reactions and subsequent delta H values, C2H6 (g) -> C2H2 (g) + 2H2 (g) delta H= 283.5 kJ H2 (g) + 1/2 O2 (g) -> H2O (g) delta H= -213.7 kJ 2CO2 (g) + 3H2O (g) -> C2H6 (g) + H2O (g) delta H= 849 kJ Find the delta H for the reaction: C2H2 (g) + 5/2 O2 (g) -> 2CO2 (g) + H2O (g)
Find the mass of ethane C2H6 required to produce 5000 kJ of heat. C2H6(g) + 7...
Find the mass of ethane C2H6 required to produce 5000 kJ of heat. C2H6(g) + 7 2O2(g) = 2CO2(g) + 3H2O(g), ∆H◦ = −1423 kJ/mol. (C2H6) = 30.07 g/mol.
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
Using the standard molar heat of combustion of hydrogen, methane, and ethane (given below), find the...
Using the standard molar heat of combustion of hydrogen, methane, and ethane (given below), find the enthalpy change for 2CH4(g) → C2H6(g) + H2(g) H2 + ½ O2 → H2O ΔHo = -285.8 kJ CH4 + 2O2 → CO2 + 2H2O ΔHo = -890.4 kJ C2H6 + (7/2)O2 → 2CO2 + 3H2O ΔHo = -1559.9 kJ
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX:...
Given the following reactions: 2 S (s) + 3 O2 (g) ⟶ 2 SO3 (g) ΔH1= LaTeX: -− 790 kJ S (s) + O2 (g) ⟶ SO2 (g) ΔH2= LaTeX: -−297 kJ What is the enthalpy change of the following reaction? 2 SO3 (g) ⟶ 2 SO2 (g) + O2 (g) ΔH3=?
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
Compounds with carbon-carbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation C,H (9) + H2(g) + C H (9) Calculate the enthalpy change for this reaction, using the following combustion data: C4H4 () + 30 (g) + 2CO3(g) + 2H2O(); AH = -1411 kJ C, H(g) + O2(g) → 2002(g) + 3H2O(l); AH = -1560. kJ H2(g) + O2(g) H2O(l); AH = -286 kJ Enthalpy change - KJ Submit Answer Try Another Version 10 item...
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