The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon
ignition or sudden impact according to the following balanced
equation:
4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g)ΔH∘rxn=−5678kJ
Calculate the standard enthalpy of formation (ΔH∘f) for
nitroglycerin.
?=kJ/mol
The explosive nitroglycerin (C3H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following bal...
explosive nitroglycerin (C3 HN3 O9) decomposes rapidly ignition or sudden impact according to the following balanced equation: 4CaHsN3 Os (12CO2 (g) 10H2O(g) 6N2(g) + O2(g) AHpR=-5678 kJ You may want to reference (Pages 277-280) Section 6.9 while completing this problem. Part A Calculate the standard enthalpy of formation (A Hë) for nitroglycerin. Express your answer using four significant figures. ν0 ΑΣφ kJ/mol ΔΗ- Submit Request Answer
3. The explosive nitroglycerin (C3H5N309) decomposes rapidly upon ignition or sudden impact according to the balanced equation: 4 C3H5N309(1) — 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(8) AHx= -5678 kJ Calculate the standard enthalpy of formation (AH) for nitroglycerin.
The explosive nitroglycerin (C3HSN3O9) decomposes rapidly upon ignition or sudden impact according to the following unbalanced equation: 5. CO2+H2O + N2 + O2() C3H5N3O90 AHODm=-5678 k Balance this equation, and calculate the standard enthalpy of formation, AHr, of nitroglycerin.
Nitroglycerin (C3H5N309) decomposes explosively upon ignition or sudden impact according to the following balanced equation: 4C3H5N30 (1) ► 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) Hºrxn--5678 kJ Compound CO2 HO AHⓇ(kJ/mol) at 298 K -393.5 -241.8 Determine whether each statement is true or false using the provided drop-down menus. 1) If 1.2 moles of C3H5N30, decompose, the energy change of the reaction (x) is -5,678 kJ. [Select 2) The reaction releases energy to the surroundings. (Select] 3)...
Assume that you have 1.15 g of nitroglycerin in a 579.5 mL steel container at 20.0 ∘C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 ∘C. The balanced equation is 4C3H5N3O9(l)→12CO2(g)+10H2O(g)+6N2(g)+O2(g) (Figure 1) Part A How many moles of nitroglycerin were in the container originally? Part B How many moles of gas (air) were in the container originally? Part C How many moles of gas are in the container after...
A 1.000 kg sample of an organic compound, C3H5N3O9, explodes and releases gases with a temperature of 1985°C at 836.0 atm. What is the volume of gas produced? (always balance equations) C3H5N3O9(s) → CO2(g) + H2O(g) + N2(g) + O2(g) The listed answers are: 5378 L, 742.2 L, 3525 L, 4730 L, 352.5 L My answer: We have: 1.000 kg --> 1.000x10^3 g =1,000 g C3H5N3O9 T= 1985C --> 1985C+273= 2258K P= 836.0 atm V=? Balanced equation: 4C3H5N3O9-->12CO2+10H2O+6N2+O2 C= 3*12.0107...
A metal object at 54.0 oC is heated by gaining 30.2 kJ of heat from the environment. The heat capacity, C, of the metal object is 6.30 kJ/ oC When 11.53 g C2H6O (g) is reacted according to the following equation, 368 kJ of heat is released. What is the ΔH of the reaction? C2H6O (g) + 3O2(g) --> 2CO2(g) + 3H2O (l) When 2.45 g of CH3OCH3 is burned at constant Pressure, 77.42 kJ of heat is given off. What is...
The standard enthalpy of formation of CO(g) is −111 kJ/mol [refer to this equation C(s) + 1/2O2(g) ⟶ CO(g)] What is the ΔHorxn of this reaction? (What is the standard enthalpy change of this reaction?) 2C(s) + O2(g) ⟶ 2CO(g) -253 kJ/mol - 222 kJ/mol -97.1 kJ/mol 534 kJ/mol 124.9 kJ/mol -50.5 kJ/mol 5 points QUESTION 2 (assume A, B, C, and D and E are chemicals) Look at these equations A + B à C ΔH° = -9 kJ/mol rxn...
Propane (C3H8)burns according to the following balanced equation: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g) Calculate ΔH∘rxnΔ for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of gaseous propane is -103.9 kJ/molkJ/mol.) Express the enthalpy in kilojoules to four significant figures.
1).From the standard enthalpies of formation, calculate ΔH°rxn for the reaction C6H12(l) + 9O2(g) → 6CO2(g) + 6H2O(l) For C6H12(l), ΔH°f = –151.9 kJ/mol (5 points) Substance ∆H°f , kJ/mol C6H12(l) –151.9 O2(g) 0 H2O(l) –285.8 CO2(g) –393.5 2).Determine the amount of heat (in kJ) given off when 1.26 × 104 g of ammonia are produced according to the equation N2(g) + 3H2(g) → 2NH3(g) ΔH°= –92.6 kJ/mol Assume that the reaction takes place under standard conditions at 25oC.