**Problem 9**: Use the Table of Thermodynamic Data on the right for the decomposition reaction:\[ 3 \text{N}_2\text{H}_4(l) \rightarrow 4 \text{NH}_3(g) + \text{N}_2(g) \]to calculate the kilojoules of heat released per one gram of N₂H₄ reacted.**Table of Thermodynamic Data**| Substance | ΔH⁰f, kJ/mol ||------------|--------------|| NH₃(g) | -46.3 || N₂(g) | 0 || N₂H₄(l) | +50.4 |The molar mass involved is: \[ M_{\text{N}_2\text{H}_4} = 32.046 \text{ g/mol} \]**Round off your answer to 3 significant figures** and enter it in the box provided with correct units:**Answer:**The heat released per one gram of N₂H₄ is: \[ \Delta q_{\text{surr}} = \](Note: Specific calculations were not provided in the image, thus the solution box is left blank for completion by the student.)

Enthalpy of a reaction is given by the change in enthalpy of products and reactants.

Page 3 of Problem 9 ( ). Use the Table of Thermodynamic Data on the right Substance AH, moi for the decomposition reaction: kJ NH,() -46.3 3N,H,0) 4NH,(g) + N2(9) to calculate the kilojoules of heat released per one gram of N,H, reacted. N,H,0) +50.4 The molar mass involved is: = 32.046 9 mol: Round off your answer to 3 sig. figs. and enter it in the box provided with correct units: The heat released per Answer: : Aqsurr %3D one gram of N,H4 is

Page 3 of Problem 9 ( ). Use the Table of Thermodynamic Data on the right Substance AH, moi for the decomposition reaction: kJ NH,() -46.3 3N,H,0) 4NH,(g) + N2(9) to calculate the kilojoules of heat released per one gram of N,H, reacted. N,H,0) +50.4 The molar mass involved is: = 32.046 9 mol: Round off your answer to 3 sig. figs. and enter it in the box provided with correct units: The heat released per Answer: : Aqsurr %3D one gram of N,H4 is

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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THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) – 2X2M (I) + 2DM2 (g) AH°F for X2D (g) = -24.4 kJ/mol AH°f for DM2 (g) = -290.7 kJ/mol AH°; for X2M (I) = -283.1 kJ/mol AH°; for M2 (g) = 0 kJ/mol
THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off the final answer to ONE decimal place. Do not include the unit.) 2X2D (g) + 3M2 (g) – 2X2M (I) + 2DM2 (g) AH°f for X2D (g) = -26 kJ/mol AH°f for DM2 (g) = -296.8 kJ/mol AH°f for X2M (1) = -286.5 kJ/mol AH°f for M2 (g) = 0 kJ/mol
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10. The following molar enthalpies of formation are given in kJ/mol: AHP[C;Hs(g)] = -104; AHP[CO2(g)] = -394; AHP[H;O(g)] = -242. (a) Calculate the molar heat of combustion of propane (C;Hs) according to the following equation: C;Hs(g) + 5 O2(g) → 3CO2(g) + 4H2O(g); (b) How many grams of propane gas must be combusted to provide enough thermal energy to heat 1.00 kg water from 22.0°C to 100.0°C? (Specific heat of water = 4.184 J/mol.K)
How many grams of CaO must be added to 50.0 mL of water to make the temperature increase from 25.0 Â°C to 58.87 Â°C? The reaction is CaO(s) + H 2O(l) ↔ Ca(OH) 2(aq) -- ΔH = -83.7 kJAssume the heat capacity of the solution is the same as pure water (4.184 J/g*Â°C), the density of the solution is 1.00 g/mL and there is no loss of heat to the surroundings.
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18. Calculate the heat of reaction at constant volume for 5.00 g C3H8 ,considering the following chemical reaction: C3H8 (g) + O2(g) --------------------> CO2 (g) + H2O (g) heat of standard formation: O2 = 0.00 kJ / mole, H2O (g) = -245 kJ / mole, CO2 = -318 kJ/mole and C3H8 = -438 kJ / mole C3H8 = 44.09 g/mole Temperature is 33 oC a. -789 kJ b. -212 kJ c. 412 kJ d. -169 kJ
How 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 = rHo = -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*Twater 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 How many moles of sodium were added to the water (in moles)?
THERMODYNAMICS: Use the given standard enthalpies of formation to calculate the AH° (in kJ) for the hypothetical reaction: (Round off final answer to ONE decimal place) 2X,D (g) + 3M2 (g) → 2X2M (I) + 2DM2 (g) AH°, for X2D (g) = -22.2 kJ/mol AH° for DM2 (g) = -293.8 kJ/mol AH°; for X,M (I) = -286.6 kJ/mol AH°r for M2 (g) = 0 kJ/mol Round your answer to 1 decimal place. Add your answer
4. What mass of propane must be burned to supply 700. kJ as heat? The thermochemical equation for the combustion of propane is: C3H8(g) + 5 O2(g) → 3 CO2(g) + 4H₂O(1) AH°-2220. kJ