what is the percent yield of a reaction in which 41.5 g of solid tungsten (VI) oxide reacts with excess hydrogen to produce metallic tungsten and 9.50 mL of water? The density of water is 1.00 g/mL.

E-85 is an alternative fuel for automobiles and light trucks that consists of 85.0% (by volume) ethanol (C2H5OH), and 15.0% gasoline.  When ethanol burns completely it produces CO2 and H2O. The balanced equation for the burning of ethanol isC2​H5​OH+3O2​-->2CO2​+3H2​OThe density of ethanol is 0.790 g/mL.   How many moles of carbon dioxide are produced by the complete combustion of the quantity of ethanol in 8.00 gallons of E-85 fuel?      _mol CO2

For the reaction: Na2CO3 + CuCl2 --> CuCO3 + 2 NaCl  If 25.7 grams of NaCO3 are required to form 25.0 g of NaCl, what is the precent yield?

For the following reaction, 4.50 grams of water are mixed with excess diphosphorus pentoxide. The reaction yields 13.7 grams of phosphoric acid. diphosphorus pentoxide(s) + water(l) phosphoric acid(aq) What is the theoretical yield of phosphoric acid? What is the percent yield for this reaction?

Phenacetin can be prepared from p-acetamidophenol, which has a molar mass of 151.16 g/mol, and bromoethane, which has a molar mass of 108.97 g/mol. The density of bromoethane is 1.47 g/mL. What is the yield in grams of phenacetin, which has a molar mass of 179.22 g/mol, possible when reacting 0.151 g of p-acetamidophenol with 0.12 mL of bromoethane?

Glucose CH2O, reacts with oxygen to give CO, and H,0. What mass of the oxygen (in grams) is required for complete reaction of 25.0 g of glucose? What masses of carbon dioxide and water (in gramy are formed? CHOg O-CO2+ H,0

For the following reaction: C3Hg(g) + O2(g) ————> CO2(g) + H2O(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams for 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

Consider the reaction: C2H4 + O2     →     CO) (Unbalanced).  If 0.96 g of C2H4 g was Used 5.2 g of CO2 produced, calculate the percentage yield in the reaction. (Hint Balance the equation first).

Calculate the theoretical yield (in grams) and percent yield in the following situations: Consider the following reaction:CO + 2 H2→CH3OH What is the theoretical yield and percent yield of CH3OH if the reaction of 2.50 g of H2with an excess of CO produces 8.00 g ofCH3OH?

Determine percent yield for the reaction.    Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(�)+O2(�)→2MgO(�) When 10.1 g of Mg are allowed to react with 10.5 g of O2, 11.6 g of MgO are collected.