a theoretical yield of 3.9 kg, and 2.8

6. A piece of iron wire has a diameter of 0.485 mm. If iron has a density of 7.86 g/cc, how long (in meters) should you cut a piece of wire to obtain 0.0214 moles of iron?

A student synthesizes alum starting with 4.924 grams of scrap aluminum. When the reaction is complete, 71.54 grams of alum are collected. What is the percent yield of this reaction? I know percent yield is actual / theoretical multiplied by 100% but I'm not sure how to identify which is theoretical or actual. Thank you for helping me!

In a neutralization reaction, 50.00 mL of 0.8500 M phosphoric acid reacts with 2.500 g of magnesium hydroxide producing magnesium phosphate and water. What is the theoretical yield of magnesium phosphate (in grams)?      2. If 5.452 g of magnesium phosphate are produced in an experiment, then what is the percent yield?

A 0.206 g piece of solid magnesium reacts with gaseous oxygen from the atmosphere to form solid magnesium oxide.  In the laboratory a student weighs the mass of the magnesium oxide collected from this reaction as 0.254 g. What is the percent yield of this reaction?

A mixture of hydrocarbons contains 38.1% octane, C,H3, 13.1% heptane, C,H16, and 48.8% decane, CoH,2. The mixture is 18 combusted in an excess of oxygen. What mass of CO, is generated from the combustion of 19.2 kg of the mixture? mass of CO,: kg

A 14.599 g14.599 g sample of CaCl2CaCl2 was added to 12.147 g12.147 g of K2CO3K2CO3 and mixed in water. A 3.571 g3.571 g yield of CaCO3CaCO3 was obtained. What is the limiting reagent? CaCO3CaCO3 K2CO3K2CO3 CaCl2CaCl2 Calculate the percent yield of CaCO3.CaCO3. yield of CaCO3=CaCO3=

Given the following decomposition reaction: 4C3H5O9N3  → O2 + 12CO2 + 10H2O +6N2. a. If 28.40 g H2O were produced, what mass of CO2 will be produced?  b. If 110.5 g of C3H5O9N3 were decomposed and the yield of the reaction is 72.3%, determine the theoretical yield and actual yield.

O STOICHIOMETRY Limiting reactants 3/5 Yah Aqueous hydrochloric acid (HCI) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium chloride (NaCl) and liquid water (H,O). Suppose 22.2 g of hydrochloric acid is mixed with 17. g of sodium hydroxide. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to 2 significant digits. II

Your crucible has a mass of 30.074 g when empty, and does not change upon heating. You add some solid iron and then weigh the crucible and iron to be 32.860 g together. You then burn the iron in the presence of oxygen following the procedure in the handout. Assume that there are no contaminates and all of the iron is converted to iron oxide. The final mass of the crucible and iron oxide is 33.961 g, which does not change upon heating. The unrounded empirical formula obtained from these measurements would be FeOX, where X is a decimal type number (not necessarily a whole number). Give the value of X in the blank below in decimal format with the correct number of significant figures.Answer: ________