In one experiment you reacted 45.7 g of Aluminum with 182.8 g of Iron (III) oxide...
In one experiment you reacted 45.7 g of Aluminum with 182.8 g of Iron (111) oxide to produce Aluminum Oxide and Elemental iron (not diatomic) (10 pts each) f) What would be your % yield be if you produced 10 g of elemental iron? g) If you produced 5 grams of aluminum oxide, how many atoms of aluminum are in the 5 grams? h) The reaction required a lot of heat to begin and it did not release any heat?...
In one experiment you reacted 45.7 g of Aluminum with 182.8 g of Iron (Ill) oxide to produce Aluminum Oxide and Elemental iron (not diatomic). (10 pts each) h) The reaction required a lot of heat to begin and it did not release any heat? Was the reaction exothermic or endothermic i) If the reaction required a lot of energy what can you infer from the activation energy?
In one experiment you reacted 45.7 g of Aluminum with 182.8 g of Iron (111) oxide to produce Aluminum Oxide and Elemental iron (not diatomic). (10 pts each) c) How many mols of Iron(III) oxide do you have? d) Which is the limiting reagent? e) How many grams of Aluminum Oxide did you produced? f) What would be your % yield be if you produced 10 g of elemental iron?
Name: Chapter 7 Quiz In one experiment you reacted 45.78 of Aluminum with 182.8 g of Iron (III) oxide to produce Aluminum Oxide and Elemental iron (not diatomic). (10 pts each) a) Write and balance the chemical formula, What type of reaction was it? b) Identify the chemical that is being reduced? c) How many mols of Iron(Ill) oxide do you have? d) Which is the limiting reagent? e) How many grams of Aluminum Oxide did you produced? f) What...
Iron (III) oxide can react with aluminum metal to produce aluminum oxide and iron metal This is called the thermit reaction and it produces so much heat that it can be used for incendiary bombs and for welding. How many grams of aluminum oxide will be produced by the reaction of aluminum with 45.8 g of iron(III) oxide?
3. Aluminum undergoes a single replacement reaction with iron (III) oxide, releasing 850.2kJ of energy. How much energy would be released if 5.0g of aluminum was reacted with an excess of iron (III) oxide? a. Is this reaction exothermic or endothermic? b. Write the AH with the correct sign: c. Write the full, balanced equation. d. Use conversion factors to calculate the energy absorbed or released.
A mixture of 10.325 g of iron (III) oxide and 5.734 g of aluminum metal is placed in a crucible and heated in a high-temperature oven, where iron and aluminum oxide is formed. How many atoms of iron is formed during this reaction? (2 pts) How much aluminum, in grams, is left over after the chemical reaction has occurred? (2 pt) a.
The thermite reaction involves aluminum and iron(III) oxide forming aluminum oxide and liquid iron. Calculate the heat released in kJ per gram of aluminum reacted. The standard enthalpy of formation for liquid iron is 12.40 kJ/mol.
The highly exothermic thermite reaction, in which aluminum reduces iron (III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe2O3(s) 2Fe(s) + Al2O3(s) AH = -850 kJ What mass of iron is formed when 725 kJ of heat are released?
The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe2O3(s) - 2Fe(s) + Al2O3(s) AH=-850 kJ What mass of iron is formed when 725 kJ of heat are released?