0
What else can I help you with?
How much energy is involved in the formation of 5 grams of rust?
The energy involved in the formation of 5 grams of rust can be calculated using the enthalpy of formation of iron(III) oxide (rust), which is -824 kJ/mol. First, convert the mass of rust to moles, then use the molar enthalpy of formation to calculate the energy involved.
How many atoms of iron rusted that weight 63.8 grams?
Rusted iron is FeO, iron oxide. 63.8 grams FeO (1 mole FeO/71.85 grams)(6.022 X 1023/1 mole FeO) = 5.35 X 1023 atoms of iron oxide -------------------------------------------
Why nails do not rust in Kerosene?
Nails do not rust in kerosene because kerosene is a hydrocarbon-based liquid that lacks oxygen, which is necessary for the rusting process to occur. Without oxygen present, the nail is protected from oxidation and therefore does not rust.
Which must be present for a piece of iron to rust?
Rusting is the reaction of iron with oxygen in the presence of water.
What does rust coloured water in the radiator mean?
Rust-colored water in the radiator typically indicates the presence of rust or corrosion within the cooling system. This can be caused by old coolant, lack of maintenance, or the presence of air or contaminants in the system. It is important to flush the system and potentially replace the coolant to prevent damage to the engine.
How many moles of rust are in a pile of rust weighing 1000grams?
This depends on the exact composition of this rust.
How much energy is involved in the formation of 5 grams of rust?
The energy involved in the formation of 5 grams of rust can be calculated using the enthalpy of formation of iron(III) oxide (rust), which is -824 kJ/mol. First, convert the mass of rust to moles, then use the molar enthalpy of formation to calculate the energy involved.
How many atoms of iron rusted that weight 63.8 grams?
Rusted iron is FeO, iron oxide. 63.8 grams FeO (1 mole FeO/71.85 grams)(6.022 X 1023/1 mole FeO) = 5.35 X 1023 atoms of iron oxide -------------------------------------------
How many grams of Fe2O3 are formed when 16.7g of Fe reacts completely with oxygen?
The rusting of iron has the reaction 4 Fe + 3 O2 equals 2 Fe2O3. So every 2 moles of iron produces 1 moles of iron oxide. 16.7 grams is .299 moles of iron. This means there are 0.149 moles of iron oxide or 23.88 grams.
What has to be present for rust?
oxegon and water
What mass of hydrogen chloride is require to react with 100 g of rust?
Taking rust to be Fe2O3, you would have the following reaction:Fe2O3 + 6HCl ==> 2FeCl3 + 3H2O100 g Fe2O3 x 1 mole Fe2O3/159.7 g = 0.626 moles Fe2O3moles HCl needed = 0.626 moles Fe2O3 x 6 moles HCl/mole Fe2O3 = 3.76 moles HCl neededMass HCl needed = 3.76 moles HCl x 36.5 g/mole = 137 g HCl needed
Does water really have to be present for rust to occur?
Yes an no. There has to be humidity in the air. So yes in the form of vapors.Iron can rust whenever oxygen is present.
What is the present past and past participle of rust?
The present tense is:I/You/We/They rust.He/She/It rusts.The present participle is rusting.The past tense is rusted.The past participle is rusted.
What substance needs to be present for rust to form?
oxygen
The formula for rust can be represented by Fe2O3 How many moles of Fe are present in 14.2 g of the compound?
To find the number of moles of Fe in 14.2 g of Fe2O3, we need to use the molar mass of Fe2O3 (molecular weight = 159.69 g/mol) and the ratio of Fe to Fe2O3. There are 2 moles of Fe in 1 mole of Fe2O3, so we find the moles of Fe in 14.2 g of Fe2O3 by: (14.2 g / 159.69 g/mol) * 2 = 0.249 moles of Fe.
How many grams of iron oxide would be formed if 2 moles of iron completely react with oxygen gas?
The mass is 80 g iron)III) oxide.
What is the metal that needs to be present for rust to occur?
FE or Iron
