What is ΔH for the explosion of nitroglycerin? (LO 9.14)2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2(g) + 6 CO2(g) + 5 H2O(g)(a) −315.0 kJ(b) −4517 kJ(c) −3425 kJ(d) −3062 kJ

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Identify the balanced chemical equation for the reaction: 2 C_3H_5(NO_3)_3(l) \rightarrow 3 N_2(g) + \frac{1}{2} O_2(g) + 6 CO_2(g) + 5 H_2O(g).

Determine the standard enthalpy of formation (\Delta H_f^\circ) for each reactant and product involved in the reaction. These values are typically found in a table of standard enthalpies of formation.

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Use the formula for the standard enthalpy change of the reaction: \Delta H_{reaction}^\circ = \sum \Delta H_f^\circ (products) - \sum \Delta H_f^\circ (reactants).

Calculate the total \Delta H_f^\circ for the products by multiplying the \Delta H_f^\circ of each product by its stoichiometric coefficient and summing them up.

Calculate the total \Delta H_f^\circ for the reactants in a similar manner, and then subtract the total \Delta H_f^\circ of the reactants from the total \Delta H_f^\circ of the products to find \Delta H_{reaction}^\circ.

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Key Concepts

Enthalpy Change (ΔH)

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ΔH < 0) or endothermic (absorbs heat, ΔH > 0). In the context of chemical reactions, calculating ΔH helps predict the energy changes associated with the formation or breaking of bonds during the reaction.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows chemists to determine the proportions of substances consumed and produced, which is essential for calculating the enthalpy change of a reaction. In this case, the stoichiometric coefficients from the balanced equation for nitroglycerin decomposition are crucial for determining the total energy change.

Standard Enthalpy of Formation

The standard enthalpy of formation is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. This value is used to calculate the overall ΔH for a reaction by applying Hess's law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps. Knowing the standard enthalpies of formation for the reactants and products allows for accurate ΔH calculations.

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Related Practice

Textbook Question

When 12.5 g of NH4NO3 is dissolved in 150.0 g of water of 25.0 °C in a coffee cup calorimeter, the final temperature of the solution of 19.7 °C. Assume that the specific heat of the solution is the same as that of water, 4.18 J/(g•°C). What is the ΔH per mol of NH4NO3? (LO 9.10) NH4NO3 (s) → NH4+ (aq) + NO3−(aq) ΔH = ? (a) +3.60 kJ (b) +23.0 kJ (c) +21.3 kJ (d) −3.60 kJ

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Textbook Question

Calculate the enthalpy change for the reactionC(s) + 2 H2(g) → CH4(g) ΔH = ?Given the enthalpy values for the following reactionsCH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH = −890.4 kJC(s) + O2(g) → CO2(g) ΔH = −393.5 kJH2(g) + 1/2 O2(g) → H2O (g) ΔH = −285.8 kJ(a) −1569.7 kJ(b) +211.1 kJ(c) −1855.5 kJ(d) −74.7 kJ

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Textbook Question

A table of standard enthalpies of formation (ΔH°f) gives a value of −467.9 kJ/mol for NaNO3(s). Which reaction has a ΔH° value of −467.9 kJ?(a) Na+ (aq) + NO3−(aq) → NaNO3(s)(b) Na(s) + N(g + O3(g) → NaNO3(s)(c) Na(s) + 1/2 N2(g) + 3/2 O2(g) → NaNO3(s)(d) 2 Na(s) + N2(g) + 3 O2(g) → 2 NaNO3(s)

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Textbook Question

A piece of dry ice (solid CO2) is placed inside a balloon, and the balloon is tied shut. Over time, the carbon dioxide sub- limes, causing the balloon to increase in volume. Give the sign of the enthalpy change and the sign of work for the sublima-tion of CO2.

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Verified step by step guidance

1. Identify the balanced chemical equation for the reaction: 2 C_3H_5(NO_3)_3(l) \rightarrow 3 N_2(g) + \frac{1}{2} O_2(g) + 6 CO_2(g) + 5 H_2O(g).
2. Determine the standard enthalpy of formation (\Delta H_f^\circ) for each reactant and product involved in the reaction. These values are typically found in a table of standard enthalpies of formation.
3. Use the formula for the standard enthalpy change of the reaction: \Delta H_{reaction}^\circ = \sum \Delta H_f^\circ (products) - \sum \Delta H_f^\circ (reactants).
4. Calculate the total \Delta H_f^\circ for the products by multiplying the \Delta H_f^\circ of each product by its stoichiometric coefficient and summing them up.
5. Calculate the total \Delta H_f^\circ for the reactants in a similar manner, and then subtract the total \Delta H_f^\circ of the reactants from the total \Delta H_f^\circ of the products to find \Delta H_{reaction}^\circ.

Key Concepts

Enthalpy Change (ΔH)

Enthalpy change (ΔH) is a measure of the heat content of a system at constant pressure. It indicates whether a reaction is exothermic (releases heat, ΔH < 0) or endothermic (absorbs heat, ΔH > 0). In the context of chemical reactions, calculating ΔH helps predict the energy changes associated with the formation or breaking of bonds during the reaction.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows chemists to determine the proportions of substances consumed and produced, which is essential for calculating the enthalpy change of a reaction. In this case, the stoichiometric coefficients from the balanced equation for nitroglycerin decomposition are crucial for determining the total energy change.

Standard Enthalpy of Formation

The standard enthalpy of formation is the change in enthalpy when one mole of a compound is formed from its elements in their standard states. This value is used to calculate the overall ΔH for a reaction by applying Hess's law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps. Knowing the standard enthalpies of formation for the reactants and products allows for accurate ΔH calculations.