Consider the following reaction: 2 H2( g)+O2( g) ⟶2 H2 O(l) ΔH=-572 kJ a. How much heat is ev

step 1 It's considered the reaction 2H2 gas, plus O2 gas, producing 2H2O. Liquid delta H here is equal

Consider the following reaction: 2 H2( g)+O2( g) ⟶2 H2 O(l) ...

Consider the following reaction: $$ 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H=-572 \mathrm{~kJ} $$ a. How much heat is evolved for the production of $1.00 \mathrm{~mol}$ $\mathrm{H}_{2} \mathrm{O}(l) ?$ b. How much heat is evolved when $4.03 \mathrm{~g}$ hydrogen is reacted with excess oxygen? c. How much heat is evolved when $186 \mathrm{~g}$ oxygen is reacted with excess hydrogen? d. The total volume of hydrogen gas needed to fill the Hindenburg was $2.0 \times 10^{8} \mathrm{~L}$ at $1.0 \mathrm{~atm}$ and $25^{\circ} \mathrm{C}$. How much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted?

Consider the following reaction:
$$
2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l) \quad \Delta H=-572 \mathrm{~kJ}
$$
a. How much heat is evolved for the production of $1.00 \mathrm{~mol}$ $\mathrm{H}_{2} \mathrm{O}(l) ?$
b. How much heat is evolved when $4.03 \mathrm{~g}$ hydrogen is reacted with excess oxygen?
c. How much heat is evolved when $186 \mathrm{~g}$ oxygen is reacted with excess hydrogen?
d. The total volume of hydrogen gas needed to fill the Hindenburg was $2.0 \times 10^{8} \mathrm{~L}$ at $1.0 \mathrm{~atm}$ and $25^{\circ} \mathrm{C}$. How much heat was evolved when the Hindenburg exploded, assuming all of the hydrogen reacted?

Key Concepts

Ideal Gas Law Application

The ideal gas law is a fundamental equation (PV = nRT) that correlates the pressure, volume, temperature, and number of moles of a gas. It is utilized to determine the amount of gas present under specified conditions, which is important when gases are reactants or products in a reaction.

Mass-to-Mole Conversions

Mass-to-mole conversions involve using the molar mass of a substance to convert a given mass into moles. This process is critical for translating measurable laboratory quantities (mass) into the amount of substance (moles) used in stoichiometric calculations.

Limiting Reactant Concept

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thereby limiting the amount of product formed. Identifying the limiting reactant is crucial when reactants are provided in non-stoichiometric amounts, as it determines the maximum yield attainable in the reaction.

Thermochemistry and Enthalpy Change

Thermochemistry is the study of energy changes, particularly heat, in chemical reactions. The enthalpy change (?H) represents the heat absorbed or released at constant pressure during a reaction. A negative ?H indicates an exothermic reaction, where energy is released to the surroundings.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation’s coefficients to relate the mole ratios of reactants and products. This concept enables you to determine how much of one substance is required or produced given a certain amount of another, serving as the foundation for quantitative analysis in chemical reactions.

Mole-to-Mole Conversions

Mole-to-mole conversions use the relationships provided by the stoichiometric coefficients in the balanced equation to convert between the amounts (in moles) of different reactants and products. This conversion is essential for linking the consumption of reactants to the formation of products.

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