INTERACTIVE EXAMPLE Using Enthalpies of Formation Nitroglycerin is a powerful explosive that forms four different gases when detonated: 2 C3H5(NO3)3() →3 N₂(g) + 1/2 O₂(g) + 6 CO₂(g) + 5 H₂O(g) Calculate the enthalpy change that occurs when 17.0 g of nitroglycerin is detonated. The standard enthalpies of formation are shown below. AH (kJ/mol) C3H5(NO3)3()-364 CO₂(g) H₂O(g) -393.5 -241.8 kJ

INTERACTIVE EXAMPLE Using Enthalpies of Formation Nitroglycerin is a powerful explosive that forms four different gases when detonated: 2 C3H5(NO3)3() →3 N₂(g) + 1/2 O₂(g) + 6 CO₂(g) + 5 H₂O(g) Calculate the enthalpy change that occurs when 17.0 g of nitroglycerin is detonated. The standard enthalpies of formation are shown below. AH (kJ/mol) C3H5(NO3)3()-364 CO₂(g) H₂O(g) -393.5 -241.8 kJ

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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Select the equation which is the correct reaction for the enthalpy of formation of potassium chlorate. O 2K(s) + Cl2(g) +3 O2(g) 2 KCIO3 (s) O K(s) + Cl2(g) + O2(g) KCI202 (s) O K(s) + 1/2 Cl2(g) + 3/202(g) KCIO3 (s) O K(s) + CI(g) + 3 O(g) → KCIO3 (s) K(s) + 1/2 Cl2(g) + 2 O2(g) KCIO4 (s)
Baking soda is sodium bicarbonate (NaHCO3). When you heat baking soda, it breaks down into sodium carbonate powder (Na2CO3), water vapor, and carbon dioxide. The enthalpy of this reaction is 129 kJ. Write a correct thermochemical equation for this reaction, explain how you came up with this equation, and explain what it tells you about the reaction.
Using Hess's Law to calculate net reaction enthalpy Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) → 2NH3(g) In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH3(g) + 50₂(g) → 4NO(g) + 6H₂O(g) ΔΗ= - 905. kJ ΔΗ= - 92. kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. kJ X S
Given the following thermochemical equations P4(s) + 6C12(g) 4PCI3(g) AH = -2439 kJ/mol 4PCI5(g) → P4(s) + 10CI 2(g) AH = 3438 kJ/mol find the AH for the reaction below, PCI5(g) → PC|3(g) + Cl2(g) O A) +249.8 kJ/mol O B) +999 kJ/mol O C) -999 kJ/mol O D) -249.8 kJ/mol
3. Hydrazine, N2H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the process in which hydrazine is formed from its elements? N2(g) + 2H2(g) → N2H4(l) Use the following reactions, enthalpy changes, and Hess’s Law N2H4(l) + O2(g) → N2(g) + 2H2O(l); ΔrH° = −622.2 kJ H2(g) + ½O2(g) → H2O(l); ΔrH° = −285.8 kJ
Consider the hypothetical thermochemical equation 3 A + B → 2 C for which AH = 63.1 kJ/mol. Which one of the following reactions would have an enthalpy change of -2×AH? Here, AH refers to the enthalpy change of the original reaction. А) С — 3/2 А + 1/2 В B) 6 A + 2 B –→ 4 C С) 3/2 А + 1/2 В — С D) 4 C → 6 A + 2 B
Given the two thermochemical equations below, find the enthalpy change for the reaction: N2H4 (l) + H2 (g) → 2 NH3 (g) delta H = ? Given: N2O4 (g) + 3 H2 (g) → 2 NH3 (g) + 2 O2 (g) delta H = – 100.96 kJ N2O4 (g) + 2 H2 (g) → N2H4 (l) + 2 O2 (g) delta H = + 41.47 kJ Select one: a. – 142.43 kJ b. – 59.49 kJ c. + 41.47 kJ d. + 59.49 kJ e. + 142.43 kJ f. none of these g. – 100.96 kJ
From the following data, C (graphite) + O₂(g) → CO₂(g) H₂(g) + —⁄- 02₂(g) → H₂O (1) CH₂(g) + 20₂(g) → CO₂(g) + 2H₂O (1) kJ ×10 Calculate the enthalpy change for the reaction below: C(graphite) + 2H₂(g) CH4 (g) Be sure your answer has the correct number of significant digits. X → ΔΗ° S rxn ΔΗ° = -285.8 rxn = -393.5 ΔΗ° = -890.4 rxn kJ mol kJ mol kJ mol
a You want to determine the value for the enthalpy of formation of CaSO4(s). Ca(s) + S(s) + 2 O₂ (g) → CaSO4(s) This reaction cannot be done directly. You know, however, that both calcium and sulfur react with oxygen to produce oxides in reactions that can be studied calorimetrically. You also know that the basic oxide CaO reacts with the acidic oxide SO3 (g) to produce CaSO4(s) with A₁ H° = -402.7 kJ. Outline a method for determining A₁H˚ for CaSO4(s), and identify the information that must be collected by experiment. Using enthalpy of formation data, confirm that AƒH° for CaSO4(s) = −1433.5 kJ/mol. What compound is formed when Ca and O2 react?
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