Nitric oxide, NO, is a product generated in automobile exhaust. What mass of NO (30.01 g/mol) can be formed from the reaction of 2.00 g NO2 (46.01 g/mol) and excess oxygen according to the equation shown below? NO2(g) + O2(g) –→ NO(g) + O3(g) O 0.769 g NO O 3.07 g NO O 15.00 g NO O 2.00 g NO O 1.30 g NO

Using the following balanced synthesis reaction for silver oxide, how many grams of oxygen are needed to completely react with 85.0 grams of silver? 4 Ag (s) + O2 (g) ----> 2 Ag2O (s) 1 mol Ag 107.87 g Ag 4 mol 02 6.022 x 1023 , 02 1 mol Ag" 85 g Ag x 1 тol O2 O 85 g Ag x 1 mol Ag 107.87 g Ag 4 mol 02 22.4 g O2 1 mol Ag“ 1 mol 02 O 85 g Ag x 1 mol Ag 107.87 g Ag 1 тol Op16.00 g О2 4 mol Ag 1 тol Oz 1 mol Ag 107.87 g Ag 1 mol 02 32.00 g O2 4 mol Ag" 1 mol 02 85 g Ag x

How many atoms of CO2 can be produced from 4.21 x 10^28 atoms of oxygen gas (O2)? 1 mol = 6.02 x 10^23 atoms

How many moles of sodium chlorate (NaCIO3) are required to produce 0.235 mol O2? 2 NaCIO3(s) – 2 NaCI(s) + 3 O2(g)

Iron(III) oxide reacts with carbon monoxide according to the equation:Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)A reaction mixture initially contains 22.35 g Fe2O3Fe2O3 and 15.54 g CO Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

A sample of a substance (containing only C, H, and N) is burned in oxygen.3.375 g of CO2, 4.935×10-1 g of H2O and 6.575×10-1 g of NO are the sole products of combustion.What is the empirical formula of the compound?   What was the mass of the initial sample burned?

What is the mass in grams of H₂ that can be formed from 54.4 grams of NH₃ in the following reaction? 2 NH₃(g) → 3 H₂(g) + N₂(g)

2 HgO(s) → 2 Hg(ℓ) + O₂(g) 4.00 grams of HgO was used in this reaction. How many moles of HgO were used?

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) → 2 NO(g) If 5.220 g N₂ is mixed with 9.660 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. g

How many moles of ammonia would be required to react exactly with 0.576 moles of copper(II) oxide in the following chemical reaction? 2 NH₃(g) + 3 CuO(s) → 3 Cu(s) + N₂(g) + 3 H₂O(g) How many moles of nitrogen gas would be produced if 4.81 moles of copper(II) oxide were reacted with excess ammonia in the following chemical reaction? 2 NH₃(g) + 3 CuO (s) → 3 Cu(s) + N₂(g) + 3 H₂O(g) What is the mass in grams of CuO that would be required to produce 13.50 moles of nitrogen gas in the following chemical reaction? 2 NH₃(g) + 3 CuO(s) → 3 Cu(s) + N₂(g) + 3 H₂O(g) How many molecules of SO₃ can be formed from 0.18 moles of O₂ (assuming excess SO₂) from the following UNBALANCED equation? SO₂(g) + O₂(g) → SO₃(g)