What is the percent yield for a reaction if we predicted the formation of 20 grams of CO gas and actually recovered only 4 grams? a 50% b 70% C 20% d 40%

Determine the total mass of the product that could be formed from the balanced reaction shown below if one starts with 4.20 g Al (26.98 g/mol) and 17.40 g iodine, I₂ (MW 253.80 g/mol). 2Al + 3I₂ → 2AlI₃     Set up the table below that represents 100% yield with the given reaction conditions..

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I would need help to answer the following question. In the chemical industry, determining the quantity of substances to be produced in chemical reactions is considered extremely important. The area of chemistry that determines the amount of reactants to be used and the amount of products to be obtained in chemical reactions is Stoichiometry. Considering the context above and your knowledge acquired during classes, for the reaction below calculate the amount of oxygen gas required to produce 13.5 moles of water, H2O(g), in the complete combustion of acetylene, C2H2(g)? C2H2(g) + O2(g) →  CO2(g) +  H2O(v)

For the following reaction: C3H8(g) + 02 ——-> CO2(g) +H20(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams of each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams

According to the following reaction, how many grams of hydrofluoric acid will be formed upon the complete reaction of 26.4 grams of water with excess silicon tetrafluoride? silicon tetrafluoride (s) + water (I) --> hydrofluoric acid (aq) + silicon dioxide (s) O58.6g O 2.9g O 14.7g 20.2g

For the following reaction, 0.497 moles of sulfur are mixed with 0.217 moles of carbon monoxide. What is the formula for the limiting reagent? What is the maximum amount of sulfur dioxide that can be produced? sulfur(s) + carbon monoxide(g) -> sulfur dioxide(g) + carbon(s)

A student was able to detect a mass increase of 0.500 grams during the reaction between Mg and O2. Oxygen was present in excess and the starting mass of Mg was 1.00 g. What is the percent yield of the reaction? O 50.0% O 90.9% O 150.% O 66.7%

how do I do this step by step?

A student heats a 2.8695g sample of a mixture that contains an unknown amount of potassium chlorate (KClO3). The KClO3in the mixture decomposes and releases its oxygen. The mass of the remaining sample residue was 2.0427g. KClO3(s) →KCl (s) + 3 O (g) a.How many grams of oxygen were in the KClO3sample? b.How many moles of oxygen atoms is this? c.How many moles of KClO3were in the original sample? d.How many grams of KClO3were in the original sample? e.What is the % of KClO3in the original sample?