Potassium chlorate, KClO3, can be decomposed by heating. 2 KClO3( s) ⟶2 KCl(s)+3 O2( g) If 465

step 1 To calculate the mass of oxygen, we first need to calculate the moles of oxygen. To calculate th

Potassium chlorate, KClO3, can be decomposed by heating. 2...

Potassium chlorate, $\mathrm{KClO}_{3}$, can be decomposed by heating. $$ 2 \mathrm{KClO}_{3}(\mathrm{~s}) \longrightarrow 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g}) $$ If $465 \mathrm{~mL}$ gas was collected over water at a total pressure of $750 . \mathrm{mm} \mathrm{Hg}$ and a temperature of $23^{\circ} \mathrm{C}$, how many grams of $\mathrm{O}_{2}$ were collected?

Potassium chlorate, $\mathrm{KClO}_{3}$, can be decomposed by heating.
$$
2 \mathrm{KClO}_{3}(\mathrm{~s}) \longrightarrow 2 \mathrm{KCl}(\mathrm{s})+3 \mathrm{O}_{2}(\mathrm{~g})
$$
If $465 \mathrm{~mL}$ gas was collected over water at a total pressure of $750 . \mathrm{mm} \mathrm{Hg}$ and a temperature of $23^{\circ} \mathrm{C}$, how many grams of $\mathrm{O}_{2}$ were collected?

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Key Concepts

Dalton’s Law of Partial Pressures

This law states that the total pressure of a gas mixture is the sum of the partial pressures of individual gases. It is used to separate the pressure contributions of the water vapor and the collected gas.

Vapor Pressure Correction

When a gas is collected over water, the measured pressure includes the pressure exerted by water vapor. Adjusting for vapor pressure is necessary to obtain the true pressure of the gas of interest.

Molar Mass Conversion

Molar mass conversion is the process of converting the number of moles of a substance into its mass by using its molar mass, which is a key final step in quantitative chemical calculations.

Stoichiometry

This concept involves using a balanced chemical equation to relate the number of moles of reactants to the number of moles of products. It forms the basis for converting between amounts of substances in chemical reactions.

Ideal Gas Law

The Ideal Gas Law (PV = nRT) relates the pressure, volume, temperature, and number of moles of a gas. It is essential for determining the quantity of gas under given conditions.

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