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- Consider the following reactions: C2H6 (g) + 7/2 O2 (g) → 2 CO2 (g) + 3 H2O (l) ΔHo = − 1541 kJ H2 (g) + ½ O2 (g) → H2O (l) ΔHo = − 286 kJ C (s) + O2 (g) → CO2 (g) ΔHo = − 393 kJ The enthalpy change, ΔHo, for 2 C (s) + 3 H2 (g) → C2H6 (g) is: A. −1541 kJ B. 469 kJ C. 862 kJ D. −103 kJ E. none of the aboveHow much did our sodium-in-water demonstration raise the temperature of water in the dessicator jar? The reaction we performed was: Na(s) + H2O(l) → NaOH(aq) + 1/2H2(g) qreaction = ΔrHo = -184 kJ/mol-rxn Assuming the dessicator jar is well insulated (like our coffee-cup calorimeter), the energy balance is: 0 = qsystem = qreaction + qwater ⇒ qreaction = -qwater qreaction = -mwater*Cwater*ΔTwater The data from the demonstration was: (a) 1.0 kg water, (b) 22.0oC, (d) Cwater = 4.18 J/g-K, (e) mNa = 0.21 g What is the molar mass of sodium, Na, in g/mol?Write the equation for the standard enthalpy of formation (ΔHf°) for solid magnesium nitrate.
- Part 1.) 4NH3 (g) +502 (g) - -- > 4 NO (g) 6H2O (g)Write the formation reactions for the compounds shown and their enthalpy of formation values. NO is already provided. rxn 1: -- 1/2 N2 (g) + 1/2 O2 (g) > NO ( g) delta H fNO = ?, rxn 2: N2 (g) + H2 (g) - - > NH3 (g) delta HfNH 3 = ?, rxn 3: H2(g) + O2 (g) - > H 20 (g) delta H fH2O = ? In the delta sheet given I found deltaHf NO +91.3 kJ/mol, deltaHfNH3 = 45.9 kJ/mol, deltaHfH2O -241.8 kJ/mol. Part 2.) Using these three formation reactions (rxn) determine the enthalpy of the rxn. deltaHrxn using Hess's law.Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 (– 2341 kJ/mol), C4H3 (- 2755 kJ/mol), and H2 (- 286 kJ/mol), calculate AH for the reaction. САНа (9) + 2 Нэ(9) —> C4H8 (9) ΔΗ kJCH, (g) 20, (g) → CO, (g) + 2 H,O (g) + Exothermic or endothermic
- Determine the enthalpy of reaction for 2CH4(g) → C2H«(g) + 2H2(g) using the equations: 2C2H6(g) + 702(g) → 4CO2(g) + 6H2O(I) AH° = -3120.8 kJ/mol CH:(g) + 202(g) → CO2(g) + 2H2O(I) AH° = -890.3 kJ/mol C2H4(g) + H2(g) → C2H6(g) AH° = -136.3 kJ/mol H2 + ½O2(g) –→ H2O(I) AH° = -285.8 kJ/molCombustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C₂ H₂ (-1300. kJ/mol), C2H6 (-1560. kJ/mol), and H₂ (-286 kJ/mol), calculate AH for the reaction ΔΗ = C₂H₂(g) + 2H₂(g) → C₂H6 (9) kJConsider the following equation: 2C2H2(g) + 5O2(g) ->4CO2(g) + 2H2O(g) + energy (a) Does the equation represent an endothermic reaction or an exothermic reaction? (b) What effect would this reaction have on the temperature of its surroundings? Compare the temperature of the surroundings before the reaction takes place to the temperature of the surroundings after the reaction takes place. (c) What does the equation communicate about the relative energy of the chemical bonds in the reactants and products? 2. Define and distinguish among the following terms: thermal energy, heat,and temperature. 3. Use the following information to answer the questions below: Q = m × c × DT Q = heat (J) m = mass (g) c = specific heat capacity (J/g · °C) DT = Tf– Ti (°C) For water, c = 4.184 J/g · °C (a) A 50.0 g sample of water at 80.0 °C is mixed in a calorimeter with a 50.0 g sample of water at 5.0 °C. What is the final…
