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MnO can act as a catalyst in certain reactions, such as the decomposition of hydrogen peroxide. However, its catalytic activity depends on the specific reaction and conditions.
CrO₄²⁻ (chromate ion) is a strong oxidizing agent because it can readily accept electrons due to its high oxidation state of chromium, allowing it to facilitate oxidation reactions. In contrast, MnO₄⁻ (permanganate ion) is a strong oxidizing agent, but MnO₄²⁻ (manganate ion) is less effective because manganese in the +6 oxidation state (in MnO₄²⁻) is less willing to accept electrons compared to chromium in CrO₄²⁻. The effective oxidation states and the stability of the resulting products after reduction contribute to the differences in their oxidizing strengths.
The anion that decolourises a small amount of permanganate on warming is the manganate ion (MnO₄²⁻) or, more commonly, the oxalate ion (C₂O₄²⁻). When oxalate is present, it reduces permanganate (MnO₄⁻) to manganese(II) ions (Mn²⁺), causing the purple color of permanganate to fade. This reaction is often used in redox titrations.
To balance the equation involving KMnO₄ and MgS, we first need to identify the correct stoichiometric coefficients for each compound. The balanced equation will have coefficients that maintain the same number of each type of atom on both sides. The correct coefficients are 2 for KMnO₄, 1 for MgS, 2 for K₂S, and 1 for Mg(MnO₄)₂. Thus, the balanced equation is: 2 KMnO₄ + MgS → K₂S + Mg(MnO₄)₂.
When manganese dioxide (MnO₂) is heated with potassium chlorate (KClO₃), it acts as a catalyst in the decomposition of potassium chlorate. The heat causes KClO₃ to break down into potassium chloride (KCl) and oxygen gas (O₂). The presence of MnO₂ speeds up this reaction, allowing the decomposition to occur at a lower temperature. The overall reaction is: 2 KClO₃ → 2 KCl + 3 O₂.
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The empirical formula for manganese oxide is MnO.
false
False. If ABC definitely equals DEF equals MNO and MNO equals PQR then ABC does not equal PQR by the transitive property.
false
MnO
mno
MnO- 4
MnO
MnO
MnO can act as a catalyst in certain reactions, such as the decomposition of hydrogen peroxide. However, its catalytic activity depends on the specific reaction and conditions.
The oxidation number of Mn in MnO is +2. This is because oxygen generally has an oxidation number of -2 and the overall compound is neutral.