2 NO + O, + 2 NO, The balanced equation for a reaction is shown. The reactants are placed in a container, and the reaction occurs. The contents of the container after the reaction has proceeded as completely as possible are repres ONitrogen O0xygen Contents of Container After Reaction Which of the following diagrams represents the original contents of the container?

For the chemical reaction given, how many grams of sulfuric acid, HS2O4, are needed to react completely with 72.5 g of sodium hydroxide, NaOH?

Magnesium oxide can be made by heating magnesium metal in the presence of the oxygen. The balanced equation for the reaction is Determine the limiting reactant for the reaction. 2 Mg(s) + O2(9) → 2 MgO(s) When 10.1 g of Mg is allowed to react with 10.6 g O2. 12.1 g MgO is collected. O Mg(s) O2(9) Submit Request Answer Part B Determine the theoretical yield for the reaction. ? Submit Request Answer Part C Determine the percent yield for the reaction. ?

What is the balanced equation for the experiment hot ice (sodium acetate)? ***For example: The decomposition of the hydrogen peroxide into water and oxygen is catalyzed by the iodide ion. 2 H2O2(aq) → 2 H2O(l) + O2(g)   This is what I have but I feel like I am missing something? Na+ [HCO3]- + CH3 - COOH ---> CH3 - COO-NA+ + H2O + CO2

Balance each of the following reaction ___ C4H8 (g)     +     ___ O2 (g)     à     ___ CO2 (g)     +     ___ H2O (g)

A compound is composed of the elements, carbon, hydrogen, and oxygen only. Combustion of the compound produces CO2 and H2OC?H?O? + O2 ➝ CO2 + H2OCombustion of a 5.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 9.157 H2O 4.498

Suppose a 500. mL flask is filled with 1.7 mol of H₂O, 0.10 mol of CO, and 0.70 mol of H. This reaction becomes possible: CO(g)+H₂O(g) CO2(g) + H2(g) I Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of CO. You can leave out the M symbol for molarity. CO H₂O CO₂ H₂ initial ☐ 0 change x equilibrium 0 ☐ G

Use the References to access important values if needed for this question. For the following reaction, 0.127 moles of barium hydroxide are mixed with 0.119 moles of sulfuric acid. barium hydroxide (aq) + sulfuric acid (aq) → barium sulfate(s) + water (l) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of barium sulfate that can be produced? Amount = moles

Suppose the following reaction was carried out in the presence of excess Al.  Al + Cl2 --->  AlCl3 How many moles of Al are consumed if 9.07 moles of Cl2 were fully reacted?

of 15 Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl(aq) + MnO₂ (s)→ MnCl₂ (aq) + 2 H₂O(1) + Cl₂(g) A sample of 39.9 g MnO, is added to a solution containing 44.5 g HCI. B d > What is the limiting reactant? E HCI O MnO₂ What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 86.1%, what is the actual yield of chlorine? D $ 4 I R C с F % 5 V T G MacBook Pro 6 7 I I Y H B - N 4 8 J I 1 M 9 K O < F H O L P command Question F { [ option 8 Cl₂ ? 1 delete