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
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Using standard enthalpies of formation, determine the enthalpy of reaction for the following: a) CaO(s) + CO2(g) → CACO3(s) b) C2H2(g) + 2H2(g) → c) 4NH3(g) + 502(g) → 4NO(g) + 6H2O(g) C2H6(g)
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