Sodium reacts with oxygen to produce sodium oxide. 4Na(s)+O2(g)→2Na2O(s) How many grams of O2 are needed in a reaction that produces 77.0 g Na2O?

How many moles of NO can be produced by the reaction of 65.00 g of NH3 with 150.0 g of O2 according to the following balanced chemical equation? 4 NH3(g) + 5O2(g) → 4NO(g) + 6 H2O(g)

How many moles of O₂ would be required to generate 13.0 mol of NO₂ in the reaction below assuming the reaction has only 69.8% yield? 2 NO (g) + O₂ (g) → 2 NO₂ (g)

How many grams of Ab O3 will be created from reacting 36.0 g of Al with a sufficient amount of O2? 4Al(s) + 302(g) → 2Al¿Os(s)

How many moles of HNO₃ will be produced from the reaction of 34.5 g of NO₂ with excess water in the following chemical reaction? 3 NO₂(g) + H₂O (l) → 2 HNO₃(g) + NO(g)

Based on the balanced reaction: 6 CO2 + 6 H2O→ 6 O2 + C6H12O6, what is the maximum number of grams of C6H12O6 that could be made by the reaction of (5.88x10^1) g of CO2 and excess water?

Oxygen is a product of the decomposition of mercury(II) oxide as shown below. 2 HgO(s) → 2 Hg(ℓ) + O₂(g) In the last question, you determined that you started with 0.0152 moles of HgO. How many moles of O₂ gas will be formed in this reaction?

Ammonium nitrate has been used as a high explosive because it is unstable and decomposes into several gaseous substances. The rapid expansion of the gaseous substances produces the explosive force. NH,NO3 (8) → N2 (g)+ O2 (g) + H2O(g) Calculate the mass of each product gas if 47.4 g of ammonium nitrate reacts. g N2 g O2 g H2O

Consider the reaction below. Calculate how much H2O (l), in grams, can be produced if 2.5 moles of H2 is allowed excess O2? 2 H2 (g) + O2 (g) à 2 H2O (l)

When 5.0 g of propane are reacted with O2, carbon dioxide and water are produced.  How many grams of H2O can be produced by the complete reaction of those 5.0 g of propane with excess oxygen?  20 g 1.1 g 8.2 g 0.45 g 2.04 g