The reaction used to produce chlorine in the laboratory is 2 KMnO4(aq)+16 HCl(aq) →2 MnCl2(aq)+5

step 1 Hi there. In this problem, we are given a rather lengthy balanced equation. So let me get that w

The reaction used to produce chlorine in the laboratory is 2...

The reaction used to produce chlorine in the laboratory is $2 \mathrm{KMnO}_{4}(\mathrm{aq})+16 \mathrm{HCl}(\mathrm{aq}) \rightarrow 2 \mathrm{MnCl}_{2}(\mathrm{aq})+5 \mathrm{Cl}_{2}(\mathrm{aq})+$ $8 \mathrm{H}_{2} \mathrm{O}(\mathrm{aq})+2 \mathrm{KCl}(\mathrm{aq}) .$ Calculate the number of grams of potas- sium permanganate, $\mathrm{KMnO}_{4}$, that are needed to produce $9.81 \mathrm{L}$ of chlorine, measured at STP.

The reaction used to produce chlorine in the laboratory is $2 \mathrm{KMnO}_{4}(\mathrm{aq})+16 \mathrm{HCl}(\mathrm{aq}) \rightarrow 2 \mathrm{MnCl}_{2}(\mathrm{aq})+5 \mathrm{Cl}_{2}(\mathrm{aq})+$
$8 \mathrm{H}_{2} \mathrm{O}(\mathrm{aq})+2 \mathrm{KCl}(\mathrm{aq}) .$ Calculate the number of grams of potas-
sium permanganate, $\mathrm{KMnO}_{4}$, that are needed to produce $9.81 \mathrm{L}$ of chlorine, measured at STP.

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Key Concepts

Molar Mass

Molar mass is the mass of one mole of a substance and is calculated from the atomic masses of the elements within a compound. It provides the necessary conversion factor to translate between moles and grams, facilitating the determination of the mass of a reactant required to produce a given amount of product.

Molar Volume of a Gas

The molar volume is the volume occupied by one mole of a gas at STP. This constant enables the conversion of gas volumes to moles, which is critical when relating gaseous product amounts to reactants in stoichiometric calculations.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to determine the relationships between reactants and products. It requires understanding the mole ratios indicated by the coefficients in the reaction, which allow for the conversion from the amount of one substance produced or consumed to the amount of another substance involved.

Standard Temperature and Pressure (STP)

STP refers to the standard conditions of 0°C (273.15 K) and 1 atm pressure, under which one mole of an ideal gas occupies a specific volume—commonly 22.4 liters. This concept is essential for converting between the volume of a gas and the number of moles when gases are involved in chemical reactions.

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