**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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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)?
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