All changes save How many moles of H2O2 are produced in the production of hydrogen peroxide when 13 grams of oxygen are used? 2 H20+02 2 H2O2 O 81 g H2O2 O 6.5 mol H2O2 O 0.81 mol H202 O 13 mol H2O2

If a student burns 0.57 grams of methane (CH4) according to the equation below, what mass of carbon dioxide will be released?   CH4 + 2 O2 --> CO2 + 2 H2O

When a hydrocarbon such as butane (C4H10) is combusted, it produces water vapor and CO2 given in the reaction below: 2 C 4 H 10 + 13 O 2 ⟶ 8 C O 2 + 10 H 2 O How many moles of O2 are required to combust 78.89 g of butane? Round to the nearest whole number.

If 18 moles of NO combine with 29 moles of H₂, how many moles of NH, can form? What is the limiting reagent? 2 NO(g) +5 H2(g) → 2 NH3(g) + 2H2O(g) Step 1: Find the number of moles of NH3 each starting material could form. 2 moles NH3 18 moles NO × 2 moles NO 18 moles NH₂ 2 moles NH3 29 moles H₂ X 5 moles H₂ 18 moles NH3 Answer Bank 2 moles NO 5 moles H₂ 2 moles NH3 2 moles H₂O Incorrect

Balance the chemical equation below using the smallest possible whole number stoichiometric.coefficients. Na(s) + O₂(g) Na₂O₂ (s) X

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?

A student was able to detect a mass increase of 0.500 grams during the reaction between Mg and O2. Oxygen was present in excess and the starting mass of Mg was 1.00 g. What is the percent yield of the reaction? O 50.0% O 90.9% O 150.% O 66.7%

When the substance shown below burns in oxygen, the products are carbon dioxide and water. How many grams of water are obtained from burning 4.76 g of this substance? g H20 mass =

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

48.0 g of solid aluminum (Al) is combined with 150.0 grams of iron (III) oxide to form 85.0 grams of aluminum oxide and some amount of iron as shown in the equation below. Calculate the percent yield of aluminum oxide.  2Al + Fe2O3 -> Al2O3 + 2Fe