No, FeO2 is not an ionic compound. It is more likely a covalent compound based on the elements it consists of (iron and oxygen). Iron can form both ionic and covalent compounds, but in the case of FeO2, it is more likely covalent due to the high oxidation state of oxygen.
Rust.
To find the mass of FeO2 for 4.2 moles, you first need to calculate the molar mass of FeO2. Iron (Fe) has a molar mass of 55.85 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol. Adding these together gives a molar mass of FeO2 of 87.85 g/mol. Therefore, the mass of 4.2 moles of FeO2 is 4.2 moles * 87.85 g/mol = 368.37 grams.
FeO2 is a solid. It is a compound composed of iron (Fe) and oxygen (O) atoms, and it typically exists in a solid form at room temperature and pressure.
To calculate the mass of FeO2 produced, we first need to find the number of moles of O2 using the ideal gas law: PV = nRT. At STP, 1 mole of gas occupies 22.4 L, so 50.0 L of O2 is 50.0/22.4 = 2.23 moles. The balanced equation for the reaction will tell you the stoichiometry needed to calculate the mass of FeO2 produced.
No, FeO2 is not an ionic compound. It is more likely a covalent compound based on the elements it consists of (iron and oxygen). Iron can form both ionic and covalent compounds, but in the case of FeO2, it is more likely covalent due to the high oxidation state of oxygen.
Rust.
inorganic
fe + 2 O ------> FeO2 iron II oxide
To find the mass of FeO2 for 4.2 moles, you first need to calculate the molar mass of FeO2. Iron (Fe) has a molar mass of 55.85 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol. Adding these together gives a molar mass of FeO2 of 87.85 g/mol. Therefore, the mass of 4.2 moles of FeO2 is 4.2 moles * 87.85 g/mol = 368.37 grams.
FEO2
FeO2 is a solid. It is a compound composed of iron (Fe) and oxygen (O) atoms, and it typically exists in a solid form at room temperature and pressure.
FeO2= is a ferric ion where FeO3- is a ferrous ion.
To calculate the mass of FeO2 produced, we first need to find the number of moles of O2 using the ideal gas law: PV = nRT. At STP, 1 mole of gas occupies 22.4 L, so 50.0 L of O2 is 50.0/22.4 = 2.23 moles. The balanced equation for the reaction will tell you the stoichiometry needed to calculate the mass of FeO2 produced.
Kind of reddish brown. FeO2 is commonly called rust.
All metals are pure elements, however do not occur in nature necessarily as "pure." Pure being defined as the singular element without added compounds for its stability. For example, Fe2+ (iron) is commonly found in nature as FeO2 (iron oxide) because iron is oxidized in the presence of air (hence the oxygen). There are a variety of elements that all need some kind of an ion (charged particle) as a supplement for the elements' stability, commonly Lithium, Sodium, Calcium and others are in complex with the "pure" element. Another common example is table salt (NaCl). Sodium metal (Na) is highly reactive with water and humidity and is also often complexed with some other element to maintain stability.
Salt peter refers to the compound potassium nitrate or sometimes sodium nitrate. both saltpeter do have a metallic element in their make up however they are not metals any more then Feo2 (rust is a metal).