The gaseous hydrocarbon acetylene, C2H2C2H2, used in welders’ torches, burns according to the following equation: 2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g) A. What is the theoretical yield, in grams, of CO2CO2, if 26.6 gg of C2H2C2H2 completely reacts? Express your answer with the appropriate units.   B. If the actual yield in part a is 64.1 g of CO2CO2, what is the percent yield of CO2CO2 for the reaction? Express your answer with the appropriate units.

Hydrazine (N2H4) can be synthesized from ammonia (NH3) and hydrogen peroxide (H2O2) in the Peroxide process. The balanced chemical equation of this reaction is shown below: H2O2 (l) + 2NH3 (l) → 2H2O (l) + N2H4 (l) If 4 moles of ammonia were mixed with an excess amount of hydrogen peroxide, how many moles of hydrazine would be produced?

Acrylonitrile is an important building block for synthetic fibers and plastics. Over 2 billion pounds of acrylonitrile are produced in the United States each year. The compound is synthesized from propene in the following reaction:2C3H6 + 2NH3 + 3O2 → 2C3H3N + 6H2OWhat mass of acrylonitrile can be prepared from 150.0 kg of propene, 600.0 kg of ammonia, and 100.0 kg of oxygen?

Consider the reaction: Br2(g) + 3F2(g) + 2BRF3(g) Calculate the theoretical yield (in grams) for BrF3(g) when 0.100 mol of Br2 (g) is reacted with 0.150 mol of F2(g).

6. An experiment that led to the formation of the new field of organic chemistry involved the synthesisof urea, CN2H4O, by the controlled reaction of ammonia and carbon dioxide:2NH3(g) + CO2(g)  CN2H4O(s) + H2O(l)What is the theoretical yield of urea when 100. g of ammonia is reacted with 100.g of carbondioxide?

Nitric Oxide can be made from the oxidation of ammonia as shown below. A reaction between 8.5 g of NH3 and 25.0 g of O₂ produces 12.0 g of NO. What is the percent yield for this reaction? 4 NH3(g) + 5O₂(g) → 4 NO(g) + 6 H₂O(g) Molar masses (in g mol-¹): NH3 17.034, 0₂ 32.00, NO 30.01, H₂O 18.016

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

Consider the following balanced equation, an important reaction in the industrial manufacture of phosphorus pentachloride:PCl3(g) + Cl2(g) → PCl5(g)This reaction has a known yield of PCl5 of 66.3%. You are a chemical engineer tasked with producingPCl5. Determine the actual mass of phosphorus pentachloride formed when you react 61.3 kg ofmolecular chlorine with an excess of phosphorus trichloride. (P: 30.97 g/mol; Cl: 35.45 g/mol)

A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water: Mg3N2 + 3H2O → 2NH3 + 3MgO   The yield of MgO is 3.60 g. What is the percent yield in the reaction?

Determine the theoretical yield of water, in grams, when 19.66 grams of O2 reacts according to the reaction below. Use two decimal places for your molar masses and use the abbreviation for the unit. C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g)