With the aid of the following balanced equation and molar masses (MM), determine the answer for the following question. 2 CpH₁ 126 18H₂0 18.0 MM 27 0₂-18 CO₂ 44.0 32.0 If 0.141g of CH are reacted with excess O₂, what is the theoretical yield (in mL) of CO₂? At the temperature and pressure at which this reaction was conducted the density of CO₂ is equal to 1.77 g/r Report the answer to 3 significant figures.

A 5.80-g sample of lead nitrate, Pb(NO3)2, molar mass = 331 g/mol, is heated in an evacuated cylinder with volume of 3.25 L. The salt decomposes when heated,  according to the equation:  2Pb(NO3)2(s) => 2PbO(s) + 4NO2 (g) + O2 (g) Assuming complete decomposition, what is the cylinder after decomposition and cooling to a temperature of 250 K? Assume PbO(s) takes a negligible volume.  Enter answer without a unit.

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.

Answer the following questions using the stoichiometric calculation in chemistry.

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N 2 (g) → 2Li 3N (s)How many moles of lithium are needed to produce 0.20 mol of Li 3N when the reaction is carried out in the presence of excess nitrogen?     0.10     0.60     0.067     1.2     0.13

I would need help to answer the following question. In the chemical industry, determining the quantity of substances to be produced in chemical reactions is considered extremely important. The area of chemistry that determines the amount of reactants to be used and the amount of products to be obtained in chemical reactions is Stoichiometry. Considering the context above and your knowledge acquired during classes, for the reaction below calculate the amount of oxygen gas required to produce 13.5 moles of water, H2O(g), in the complete combustion of acetylene, C2H2(g)? C2H2(g) + O2(g) →  CO2(g) +  H2O(v)

A materials scientist has created an alloy containing aluminum, copper, and zinc, and wants to determine the percent composition of the alloy. The scientist takes a 12.849 g sample of the alloy and reacts it with concentrated HCl. The reaction converts all of the aluminum and zinc in the alloy to aluminum chloride and zinc chloride in addition to producing hydrogen gas. The copper does not react with the HCl. Upon completion of the reaction, a total of 10.4 L of hydrogen gas was collected at a pressure of 724 torr and a temperature of 27.0 °C. Additionally, 2.836 g of unreacted copper is recovered. Calculate the mass of hydrogen gas formed from the reaction. mass: ----- g Calculate the mass of aluminum in the alloy sample. mass: ---- g What is the mass percent composition of the alloy? Cu: -----% Zn: ----% Al: -----%

Determine the grams of ammonia produced when 1.15 g of hydrogen H is reacted with 3.75 g of nitrogen N to produce ammonia (NH) according to the following chemical equation: 3H + N → 2NH

You have 22.2 g of the compound C2Hx, where x is the maximum number of hydrogens that can fit around two carbon atoms and still create a stable Lewis dot structure. If you allow all of this sample to react with excess oxygen and then allow the products to cool to room temperature, how many moles of liquid product will you have?

Potassium chlorate, KClO 3 , decomposes upon heating in the presence of a catalyst according to the reaction below. 2KClO 3 (s) 2KCl(s)+3O 2 (g) In a certain experiment 40.0gKClO3 is heated until it completely decomposes. The experiment performed and the oxygen gas is collected and its mass is found to be 10.8g . What is the percent yield? Answer in standard notation, rounded to the nearest tenth of a percent