Identify 2 things that could happen during an experiment to cause tthe actual yeild to be lower than the theoretical yield.

Solutions containing 5.07 g of aluminum chloride and 2.71 g of silver nitrate are combined to form 1.00 g of solid product. What is the percent yield in this reaction? Note: to receive full credit, your work must also show the limiting reactant and theoretical yield for the reaction, clearly labeled a ip Design Using Autoriesk Redt 20 立

TReview Topics [Rererences Use the References to access important values if needed for this question. Furnace O absorber CO, absorber Sample A 10.08 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 14.30 grams of CO, and S.782 grams of H,0 are produced. In a separate experiment, the molar mass is found to be 62.07 g mol. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H. O empirical formula = molecular formula = Previous

Given the equation 2 NH3 -->  N2 + 3 H2, convert 5.25 mol N2 to moles of H2.  Round to the nearest 0.01, and remember to include units (properly abbreviated) and substance in your answer!

Q3 involves the reaction: Copper(II) chloride reacts w/sodium nitrate to produce copper(II) nitrate and sodium chloride. ЗА 3B I20 0a of connor/// oblarido codiumwitrato, whatmaes of oodium-chlorido-io-formod? 3C. What is the mu-. nbont2 3D. How many moles of copper(II) nitrate are formed? What mass of excess reactant is left over? ЗЕ.

O O O O The reaction bctween A, (two large red spheres) and B, (two small blue spheres) to produce AB is shown in the diagram. Determine the limiting reactant for the reaction. no limting reactant AB B2

An organic compound has a gram molecular weight of 372 g/mol, and its composition is 38.6% carbon, 9.76% hydrogen, and 51.56% oxygen. Determine (a) the empirical formula (b) the molecular formula.   C H O Mass of element (in g) (assuming 100 g of compound) 1._38.6_ 2._9.76__ 3._51.56_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____     Molecular weight of empirical formula 12._____     Molecular weight of compound / Molecular weight of empirical formula 13._____     True formula = C12H36O12

The reaction of 44.1 g of Cr203 with 35.0 g of AlI produced 25.6 g of Cr. 2Al + Cr203 --> Al203 + 2Cr 2. the percent yield of chlorine trifluoride?

How many moles of NH, can be produced from 2.71 moles of nitrogen in the following reaction: N, (9) + 3 H, (g) → 2 NH, (9) MacBook Pro Psc 888 @ # $ % & 1 2 3 4 6 7 Q W E R Y U A S D F * 00

A 60.5 mL sample of a 0.104 M potassium sulfate solution is mixed with 35.5 mL of a 0.100 M lead (II) acetate solution and the following precipitation reaction occurs: K2SO4 (aq) + Pb(C2H3 O2)2 (aq)→2KC₂ H3 O2 (aq) + PbSO4(s) The solid PbSO4 is collected, dried, and found to have a mass of 0.993 g. Determine the limiting reactant, the theoretical yield, and the percent yield.