Question

Consider the chemical reaction: $$ 2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) $$ How many moles of $\mathrm{H}_{2} \mathrm{O}$ are required to form $1.3 \mathrm{~L}$ of $\mathrm{O}_{2}$ at $325 \mathrm{~K}$ and $0.988 \mathrm{~atm} ?$

Name: Problem 90, Chapter 11: Introductory Chemistry Essentials
Uploaded: 2020-09-01T04:06:46-08:00
Duration: 1 min 57 s
Channel: Madeline Currie
Description: Consider the chemical reaction: 2 H2 O(l) ⟶2 H2(g)+O2(g) How many moles of H2 O are required to form 1.3 L of O2 at 325 K and 0.988 atm ?

   Consider the chemical reaction:
$$
2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g)
$$
How many moles of $\mathrm{H}_{2} \mathrm{O}$ are required to form $1.3 \mathrm{~L}$ of $\mathrm{O}_{2}$ at $325 \mathrm{~K}$ and $0.988 \mathrm{~atm} ?$

Introductory Chemistry Essentials

Tro, Nivaldo J. 5th Edition

Chapter 11, Problem 90

Instant Answer

Solved by Expert Madeline Currie

09/01/2020

Step 1

The ideal gas law is given by: PV = nRT Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature. Given: P = 0.988 atm V = 1.3 L T = 325 K R = 0.0821 L atm / (mol K) (ideal gas constant) We need Show more…

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Consider the chemical reaction: $$ 2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) $$ How many moles of $\mathrm{H}_{2} \mathrm{O}$ are required to form $1.3 \mathrm{~L}$ of $\mathrm{O}_{2}$ at $325 \mathrm{~K}$ and $0.988 \mathrm{~atm} ?$

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Key Concepts

Ideal Gas Law

The ideal gas law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas through the equation pV = nRT. It allows for the calculation of any one of these variables if the others are known, making it extremely useful for problems involving gases under various conditions.

Chemical Stoichiometry

Chemical stoichiometry involves using the balanced chemical equation to determine the ratios in which reactants and products participate in a reaction. This concept is crucial for converting between the amounts of different chemical species, such as determining the number of moles of a reactant needed to produce a given amount of product using the mole ratios provided by the balanced equation.

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