The reaction between aluminum and iron(III) oxide can generate temperatures approaching 3000°C and is used in welding metals: 2Al + Fe,O3 → A1½O3 +2Fe In one process, l12 g of Al are reacted with 601 g of Fe,O3. Calculate the mass (in grams) of Al,03 formed, and determine the amount of excess reagent left at the end of the reaction. mass of Al,0z formed: amount of excess reagent left:

Write a balanced chemical equation based on the following description: solid tetraphosphorus (P₄) reacts with oxygen gas to produce solid tetraphosphorus decoxide. P4(s)+O2(g)_

One of the reactions in the Solvay Process involves the reaction of calcium oxide with water toproduce slaked lime (calcium hydroxide).CaO(s) + H O2 (l) - Ca(OH)2 (s)A lab technician performs the experiment and uses 54.8 g of calcium oxide to react with a setamount of water. When the reaction is completed, the technician uses a filtration apparatus tocollect the mass of calcium hydroxide produced.    The following data is recorded:Mass of filter paper: 1.24 gMass of filter paper and solid: 68.04 g What is the theoretical mass of calcium hydroxide that is predicted to be produced? What mass of precipitate was collected in this experiment? What is the percent error? Comment on the validity of the results

Methanol has tremendous potential to be used as an alternate fuel. Carbon monoxide gas reacted with hydrogen gas can be used to produce methanol. A student reacted 32.9 g of H2(9) with excess CO(9) to produce methanol. If his percent yield was 47.7%, calculate the mass (in g) of CH3OH(1) that he collected in the experiment. Hint: Write a balanced chemical reaction equation. Do not show your work in the space provided. Record only your final answer with the correct number of significant digits and the proper units.