The reaction between aluminum and iron (Il) oxide is used in the welding process. If 120 g of Al are reacted with 300 g of Fe20s, determine the following: a Balanced chemical equation for the reaction  b) Limiting and excess reactants  c) % excess of the ER supplied  d) Mass balance for the reaction  e) Mass of metallic iron produced if the efficiency of the reaction is just 85.5%

How many grams of pure sulfuric acid could could be theoretically obtained from 762 g of natural iron pyrite (FeS2) according to this unbalanced reaction? _FeS2+_H2O+_O2—> _Fe2O3+_H2SO4

0.529 47.629 1. Initial mass of copper 2. Mass of copper and evaporating dish 3. Mass of evaporating dish 4. Mass of recovered copper 5. Percent yield (show cafcuntions) 6. Describe the reaction Cu(s)+HNO3(aq)→. 7. Describe the reaction Cu(NO3)2(aq)+NaOH(aq)→. 8. Describe the reaction Cu(OH)2(s)-A. 9. What are you removing by this washing? 10. What copper compound is present in the beaker? 11. Describe the reaction CuSO4(aq)+Zn(s) or CuSO4(aq)+ AI(s). 12. What is present in solution? 13. What is the gas? 14. How do you know? 15. What are you removing by washing? 16. What color is your copper sample? 17. Is it uniform in appearance? 18. Suggest possible sources of error in this experiment.

Data and calculations Balance the reaction first Mass (g ) Crucible ( empty) 48.11 Sample 1.00 Crucible ( after heating ) 48.81 Cuo ( actual in g) 0.70 Cu2CO3 (OH)2 221 g mol molar mass Cuo molar mass 79.5 g mol Mol Cuo produced 0.0088 mol ( actual in mol ) Mol sample used 0.0045 mol Mol Cuo calculated ( Theoretical yield in mol ) g Cuo ( Theoretical yield in g) Percent yield

A compound containing uranium and fluorine with mass 1.760 g wastreated with excess calcium nitrate to precipitate all of the fluorine. The precipitate of CaF2 had a mass of1.170 g. What is the experimental percent by mass of fluorine in the original uranium sample?

A common demonstration in chemistry courses involves adding a tiny speck of magnesium(IV) oxide to a concentrated hydrogen peroxide H2O2 solution Hydrogen peroxide is unstable and it decomposes quite spectacularly under these conditions to produce get oxygen gas and steam magnesium (IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction she was the balance equation for the decomposition reaction of hydrogen peroxide

3. A student mixes 100.0 mL of a 0.100 M solution of potassium phosphate with 100.0 mL of a 0.125 M solution of copper (II) sulfate and obtains a blue solid. (a) Write the balanced chemical equation for the reaction including physical states. (b) Determine the limiting reagent. (c) Calculate the number of moles of the excess reagent after the reaction is completed. Record servation

Given the following equation: , Ag were produced, how many atoms of Cu reacted? Cu + __ AGNO, →. Cu(NOs)2 + Ag If 89.5 grams of Answer: Molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron(III) oxide and coke (pure carbon). If 25.0 grams of pure Fe2O3 are used, how many molecules of carbon monoxide can be produced? Fe:Os +. Fe + _CO Answer: Given the following equation: NaClO3 - NaCl + , O2 How many grams of NaCl are produced when 80.0 Liters of O2 are produced at STP? Answer:

what is the balanced equation for Phosphorus triiodide is formed from elements?