The explosive nitroglycerin (C3 H5N3O9) decomposes rapidly upon ignition or sudden impact according to the following balanced equation: 4C3 H5N3 09 (1)→ 12CO2(g) + 10H₂O(g) + 6N2(g) + O2(g) A H-5678 kJ The heats of formation for carbon dioxide and water are AH (CO₂) = -393.5 kJ/mol and AH (H₂O) = -241.8 kJ/mol, respectively.

Q: Given that the molar enthalpy of combustion for propan-1-ol, C3H7OH(l), is –2008.6 kJ/mol,  what is…

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Q: Equation A: 1/2 N2 (g) = 1/2 O2 (g) = NO (g) H=90.3 Equation B: 2 NOCl (g) = N2 (g) + O2 (g) + Cl2…

A: Since, The standard enthalpy of the formation is defined as change of enthalpy of 1 mol of the…

Q: 2. Write the thermochemical equation when one mole of nitrogen gas, N, reacts with one mole of…

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Q: A chemist measures the enthalpy change AH during the following reaction: 3 N2(g) + 8 H,(9g)–4 NH3(g)…

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Q: When 3 moles of C is formed, what is the change in enthalpy? 3A + 6B + 5 kJ → 2C

A: Answer given below

Q: A student performed the procedure described in the lab manual using 48.9 mL of 1.0 M HCl and 49.9 mL…

A: Given, Acid taken: 48.9 mL of 1.0 M HCl Base taken: 49.9 mL of 1.0 M NaOH Temperature change: (24.7…

Q: 1/2 N₂(g) + 1/2 O₂(g) → NO(g) kJ/mol-rxn Enthalpy change =

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Q: with 2 mol O2 (g) to produce 1 mol CO2 (g), 2 mol H2O(l), ​and 890 kJ of heat. Write a…

A: when any substance which burns in presence of oxygen that reaction is called as combustion reaction.…

Q: Given the following equation, CaO(s) + H2O(l) → Ca(OH)2(s) ΔH°rxn = −64.8 kJ/mol how many grams of…

A: We are given the reaction CaO(s) + H2O(l) → Ca(OH)2(s) ΔH°rxn = −64.8 kJ/mol And we need to…

Q: For a particular isomer of Cg H₁8, the combustion reaction produces 5108.7 kJ of heat per mole of Cg…

A: We have to calculate the standard enthalpy of formation of C8H18(g).

Q: 2. surrou. Calculate the enthalpy change to be expected for the reaction NaCl(s)→ NaCl(aq) where (s)…

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Q: Using the information provided, determine the enthalpy (in kJ/mol) for the reaction C₃H₈ (g) + 5 O₂…

A: Given,            ∆Hf°C3H8(g) = -108.4  KJ/mole.             ∆Hf°O2(g) = 0  KJ/mole.…

Q: When a sample of Mg is combusted in a bomb calorimeter, 25.4 kJ of energy as heat is evolved. The…

A: Assuming the final temperature of water and bomb calorimeter in equilibrium is T. Hence the change…

Q: Calculate the number of grams of Mg needed for this reaction to release enough energy to increase…

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Q: D4, is used Calculate 10, from 25 perature of heat lorate is

A: Heat(Q) = mass(m) • specific heat capacity (C) • ( T2 - T1 )  Where : specific heat capacity =…

Q: Use reaction stoichiometry to calculate enthalpy change. The following reaction is exothermic. 2…

A: Basic Rule for find the Enthalpy change in new reaction. (1)  If we multiply by any number in a…

Q: Consider the formation of molecular hydrogen H₂ from hydrogen atoms: H(g) + H(g) → H₂(g). Indicate…

A: Endothermic :  The reaction in which heat is absorbed by the reaction to break bonds or to go…

Q: A student performed the procedure described in the lab manual using 49.9 mL of 1.0 M HCI and 49.3 mL…

A: Molarity of HCl = 1.0 MVolume of HCl: 49.9 mLMolarity of NaOH = 1.0 MVolume of NaOH = 49.3 mLInitial…

Q: Consider the reaction of chlorine with water vapor, H₂O(g) to form hydrogen chloride and oxygen: 1/2…

A: Enthalpy change of a reaction is a state function. If we reverse a chemical reaction than the sign…

Q: The standard enthalpy of formation (ΔH°f) for HNO3 (l) is –173.22 kJ/mol.  Which of the following…

A: The standard enthalpy of formation of compound is change of enthalpy during the formation of  1 mole…

Q: Acetic acid, CH3 CO₂H, is made industrially by the reaction of methanol and carbon monoxide.…

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Q: To determine the specific heat of a newly created, highly conducting material, a 704.8 mg sample of…

A: Mass of sample = 704.8 mg  Heat supply = 35.548  J  Initial temperature = 297.05 k  Final…

Q: e enthalpy change

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Q: The standard enthalpy change for the following reaction is -467 kJ at 298 K. Na(s) + 1/2 N2(g) + 3/2…

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Q: You wish to find the enthalpy for the reaction 6 Gel (s) + 14 NHI (s) → 3 Ge:H6 (1) + 7 N2 (g) + 38…

A: The enthalpy for the first reaction is determined as follows. 2Ge (s)+3H2g→Ge2H6l  ∆H=137.3 kJ/mol,…

Q: Using the equations 2 H: (g) + O2 (g) → 2 H2O (1) AH° = -572 kJ/mol Ca (s) + ½ O2 (g) → CaO (s) AH°…

A: The first chemical reaction is, 2H2g+O2g→2H2Ol                 ∆H°=-572 kJ/mol......(1) The second…

Q: CHEMISTRY (Please write the complete solution legibly. Choose the correct answer. No long…

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Q: Consider the hypothetical thermochemical equation 3 A + B → 2 C for which ΔH = 58.7 kJ/mol. If the…

A: The objective of the question is to find out the quantity in moles of C that would be produced when…

Q: You add some of the white crystals to a small test tube filled with water. The water in the test…

A: This can be calculated by specifi heat formula, CP = (dH/dT)P dH = Enthalpy change  dT = Temperature…

Q: Calculate the standard enthalpy for the reaction: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), given the…

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Q: Determine the enthalpy of reaction: 2NH3(g) + 2CH4(g) + 302(g) → 2HCN(g) + 6H₂O(l) Reactions…

A: We can calculate enthalpy of reaction by reversing reaction 1 and 2 and add equation 1,2,3 and 4…

Q: A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 22.4 mL of 6.45 M hydrochloric g…

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Q: A calorimeter holds 55 g water at 21.0°C. A sample of hot iron is added to the water. The final…

A: Given, Mass of water, m = 55g Temperature, T1 = 21.0oC Temperature, T2 = 24.0oC. Specific heat of…

Q: When 1.42 g of iron reacts with 1.80 g of chlorine, 3.22 g of iron(II) chloride (FeCl2, molar mass =…

A: Iron reacts with chlorine to form iron(II) chloride. When 3.22 g of  is formed, 6.8 kJ of heat is…

Q: In an industrial process to produce ammonia (NH3); nitrogen, N2, reacts with hydrogen, H2, the…

A: Ammonia can be produced in an industry with the help of nitrogen and hydrogen gas, and this process…

Q: 150.0 mL of dilute hydrochloric acid is placed in a coffee cup calorimeter. The initial temperature…

A: In the given question we have to calculate the final temperature of the solution, First of all, we…