2. Methane (CH4) Molar Mass= 16.04 g/mol) is one of the greenhouse gases. If 35.28 g of CH4 is released in the atmosphere, how many molecules of CH4 are added in the atmosphere? 3. Ethyl butanoate (C3H7COOC₂H5) is the substance responsible for the aroma of pineapple. If 95 g of it was extracted how much in number of moles was extracted?

2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol   NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.

What is the mass in grams of phosphorus trichloride that can be formed from 232.6 grams of chlorine gas based on the balanced chemical equation?  balanced chemical equation: P4(s) + 6 Cl2(g)-> 4PCl2(g)

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

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To produce zinc metal, carbon monoxide reacts with zinc (I1) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 → 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of ZnO? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).

If exactly 4.089 moles of propanol (C3H8O)  is combusted in the presence of excess oxygen what is the mass of O2 used in the reaction? The molecular weights of all reactants and products are: C3H8O: 60.09 g/mol O2: 31.998 g/mol H2O: 18.016 g/mol; CO2 : 44.01 g/mol. Enter your answer in the units of g, do not enter the unit itself.

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1. _Al + _02 > Al203 Solid aluminum and oxygen gas combine in a synthesis reaction. 4.80mol of powdered aluminum is placed into a container with 3.00 mol of oxygen. How many moles of solid aluminum oxide will be formed? What is the excess reactant? 2. Fe + H20 > Feз04 + H2 a. When 36.0g of H20 is mixed with 167g of Fe, what mass in grams of Iron oxide is produced? b. Which is the limiting reactant? 3. _CS2 + _02 → _SO2 + _CO2 If 1.60 mol of carbon disulfide gas burns with 5.60 mol of oxygen, what is the maximum amount (in grams) of CO2 that can be produced?

Consider the following balanced chemical equation.  What is the maximum mass (in grams) of water that can be produced from the combustion of 20.0 grams of ethanol with 17.0 grams of oxygen?  Round your answer to the nearest 10th of a gram. C2H5OH (g)    +    3O2(g)     →    2CO2(g)    +    3H2O(g)