How will the reaction be written when solid phosphorus is combined with oxygen gas to form diphosphorus pentoxide?

When exposed to air, aluminum metal, AlAl, reacts with oxygen, O2O2, to produce a protective coating of aluminum oxide, Al2O3Al2O3, which prevents the aluminum from rusting underneath. The balanced reaction is shown here: 4Al+3O2→2Al2O3 a) What is the theoretical yield of aluminum oxide if 3.00 molmol of aluminum metal is exposed to 2.55 molmol of oxygen? Express your answer with the appropriate units.

1. Many metals react with halogens to give metal halides. For example, iron reacts with chlorine to give iron (II) chloride, FeCl2. Fe(s) + Cl2(g) FeCl2(s). Beginning with 10.0 g iron, what mass of Cl2, in grams, is required for complete reaction? What quantity of FeCl2, in moles and in grams, is expected? 2. Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield? C3H8(g) + 3 H2O(l) 3 CO(g)+ 7 H2(g). 3. What volume of 0.812 M HCl, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence point? NaOH(aq) + HCl(aq) : H2O(l) + NaCl(aq)

A side reaction in the manufacture of rayon from wood pulp is 3CS2+6NaOH→2Na2CS3+Na2CO3+3H2O  How many grams of Na2CS3 are produced in the reaction of 92.5 mL of liquid CS2 (d = 1.26 g/mL) and 2.61 mol NaOH? Express your answer with the appropriate units.

12. 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.

The last step in the production  of nitric acid is represented by the following equation: 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) Calculate the moles of nitric acid produced when 4.43 mol of nitrogen dioxide react with excess water. Record only your final answer rounded to the correct number of significant digits and include proper units     Pure methanol, CH3OH(l), combusts very quickly. 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) If 46.5 mol of methanol undergoes complete combustion, what mass of water, in kilograms, will be produced? Record only your final answer rounded to the correct number of significant digits and include proper units.

Ammonia (NH3) is an important compound since it is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured industrially by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) + H2(g) ⇌ NH3(g) When 0.120 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places  c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places)   d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places)  Blank 4. Fill in the blank, read surrounding text. mol d. What mass of ammonia can be produced from the limiting reactant? (only 3 decimal places