Passage Potassium permanganate (KMnO 4 ) is a highly reactive inorganic salt that appears as granular dark purple crystals, nearly black in color. Due to its useful chemical properties and the fact that its reactions typically do not produce compounds that are toxic, KMnO 4 is employed in a variety of applications, including use as a topical skin disinfectant, an antifungal agent, a fire starter, and a disinfectant for drinking water.KMnO 4 is widely used as an alternative water treatment agent both to disinfect drinking water and to remove undesirable dissolved iron and sulfur compounds. The crystals are highly soluble in water and form bright pink aqueous solutions that provide a visual indication of the presence of KMnO 4 treatment residual. As a drinking water disinfectant, a KMnO 4 concentration of 1 mg/L is recommended unless higher levels of contamination are indicated by the absence of a pink residual.Industrial production of potassium permanganate is accomplished in two steps. In step 1, manganese(IV) oxide (MnO 2 ) is heated with potassium hydroxide in the presence of oxygen to produce potassium manganate (K 2 MnO 4 ), as outlined in Reaction 1.2 MnO 2 + 4 KOH + O 2 → 2 K 2 MnO 4 + 2 H 2 OReaction 1In step 2, the potassium manganate is then converted into potassium permanganate electrochemically according to Reaction 2.2 K 2 MnO 4 + 2 H 2 O → 2 KMnO 4 + 2 KOH + H 2 Reaction 2 -How many moles of O₂ are consumed if 1.8 kg of MnO₂ (MM = 86.9 g/mol) are used in Reaction 1?

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Quizplus · Accepted Answer

11ecba2d_11da_5b07_a3bf_b1696cfb31e6_MD0008_00 The molar mass of a compound is the amount of mass contained in 1 mole of the compound (grams per mole) and can be used to convert the mass of a compound to the number of moles. The reactants and/or products of a particular reaction are related to one another by the mole ratios from the balanced reaction equation. For Reaction 1, the number of moles of MnO₂ present in the reaction can be calculated by dividing the given mass of MnO₂ (1.8 kg = 1800 g) by its molar mass: (1800 g MnO₂) / (86.9 g/mol) = 20.7 moles MnO₂ reacting Reaction 1 is balanced and shows that 1 mole of O₂ is consumed for every 2 moles of MnO₂ that react. Applying this ratio, 20.7 moles of MnO₂ consumes half as many moles of O₂: (20.7 moles MnO₂) × (1 mol O₂) / (2 mol MnO₂) = 10.4 mol O₂ consumed (Choice A) If the mass of MnO₂ is not converted from kilograms to grams, 0.010 mole is obtained. (Choice C) If a 1:1 mole ratio between MnO₂ and O₂ is used rather than a 2:1 ratio, 20.7 moles is the result. (Choice D) If a 2:1 mole ratio between MnO₂ and O₂ is inverted, resulting in multiplication instead of division by 2 during the calculation, 41.4 moles is obtained. Educational objective: Given the mass of a compound sample, the number of moles present in the sample can be determined using its molar mass (the amount of mass present in 1 mole of a substance). Relating a known number of moles of a reactant to a balanced reaction equation, mole ratios can be applied to determine the number of moles of one chemical species relative to the number of moles of another chemical species in the reaction.

Passage Potassium Permanganate (KMnO4) Is a Highly Reactive Inorganic Salt That

Passage Potassium Permanganate (KMnO₄) Is a Highly Reactive Inorganic Salt That