solid potassium chlorate $\left(\mathrm{KClO}_{3}\right)$ was decomposed by the following reaction:
$$
2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)
$$

The oxygen was collected by displacement of water at $22^{\circ} \mathrm{C}$ and pressure 754 torr. The volume of the gas collected was $0.650 \mathrm{~L}$, and the vapor pressure of water at $22^{\circ} \mathrm{C}$ is 21 torr.
Calculate the partial pressure of $\mathrm{O}_{2}$ in the gas collected and the mass of $\mathrm{KClO}_{3}$ decomposed.

Question

solid potassium chlorate $\left(\mathrm{KClO}_{3}\right)$ was decomposed by the following reaction:
$$
2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)
$$

The oxygen was collected by displacement of water at $22^{\circ} \mathrm{C}$ and pressure 754 torr. The volume of the gas collected was $0.650 \mathrm{~L}$, and the vapor pressure of water at $22^{\circ} \mathrm{C}$ is 21 torr.
Calculate the partial pressure of $\mathrm{O}_{2}$ in the gas collected and the mass of $\mathrm{KClO}_{3}$ decomposed.

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Calculate the partial pressure of O₂**: To find the partial pressure of O₂, subtract the vapor pressure of water from the total pressure. Use the formula $P_{ ext{O}_2} = P_{ ext{total}} - P_{ ext{H}_2 ext{O}}$. ‖ ‖ 2 ⋮ **Calculate moles of O₂**: Use the ideal gas law rearranged to solve for moles: $n = \frac{P_{ ext{O}_2}V}{RT}$. Convert the pressure from torr to atm by dividing by 760, and use R = 0.0821 L·atm/(mol·K). Convert the temperature to Kelvin by adding 273.15 to the Celsius temperature. ‖ ‖ 3 ⋮ **Determine the mass of KClO₃ decomposed**: Use the stoichiometry of the balanced equation to find the moles of KClO₃ that decomposed. Since 2 moles of KClO₃ produce 3 moles of O₂, use the ratio $\frac{2}{3}$ to calculate the moles of KClO₃. Then, multiply by the molar mass of KClO₃ to find the mass. ‖ ∻1 Answer∻ ⚹ [Insert partial pressure of O₂ here] ⚹ ∻2 Answer∻ ⚹ [Insert mass of KClO₃ decomposed here] ⚹ ∻Key Concept∻ ⚹ Dalton's Law of Partial Pressures and the Ideal Gas Law are essential for solving gas collection problems. ⚹ ∻Explanation∻ ⚹ Dalton's Law is used to calculate the partial pressure of a gas collected over water, and the Ideal Gas Law is used to determine the amount of gas in moles, which can then be related to the stoichiometry of the chemical reaction. ⚹◊What is the formula to calculate partial pressure of a gas in a mixture?⍭ Generate me a similar question◊

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