How many moles of ethanoic acid (CH3COOH) are formed when 1799.22 g of ethanoyl chloride (CH3COCl , molar mass = 78.5 g/mol) are hydrolyzed (assuming that the reaction went to completion)? Give your answer to three significant figures. CH3COCl (l) + H2O (g) → CH3CO2H (g) + HCl (g)

[References] Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas (CH4) by the following process: Pt 2NH3 (g) + 30,(9) + 2CH, (9) → 2HCN(g) + 6H,0(g) Hydrogen cyanide is used to prepare sodium cyanide, which is used in part to obtain gold from gold-containing rock. If a reaction vessel contains 5.96 g NH3, 14.0 g O2, and 6.67 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written? Mass = НCN

What type of reaction is this? 2K(s) + Cl:(g) → 2KCI(s) * Synthesis Decomposition Combustion Single Replacement O Double Replacement

Consider the following equation: 4 NH3 (g)   +   5 O2 (g)   →   4 NO (g)   +   6 H2O (l) When 6.97 moles of ammonia (NH3) react with excess oxygen, calculate the total number of moles of products. You do not need to include units with your answer.  Notice that this question is a bit different.  You are asked for the sum of both products.

Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. Do 6.P $₁₂H₁ (1) + O₂(g) → SiO₂ (s) + H₂O(l) ? 19 X S

The balanced equation for the combustion of butane, CAH10, is shown below. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 CAH10(g) + 13 02(g) --> 8 CO2(g) + 10 H20(1) 58.124 32 44.011 18.016 How many liters of oxygen gas would be necessary to burn 18.2 g of butane?

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 7.8kg of octane burned.

What is the mass in grams of CO₂ that can be produced from the combustion of 4.06 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3C4H6O3) with salicylic acid (C7H6O3C7H6O3) to form aspirin (C9H8O4C9H8O4) and acetic acid (C2H4O2C2H4O2). The balanced equation isC4H6O3+C7H6O3→C9H8O4+C2H4O2C4H6O3+C7H6O3→C9H8O4+C2H4O2In a laboratory synthesis, a student begins with 3.10 mLmL of acetic anhydride (density=1.08gml−1density=1.08gml−1) and 1.23 gg of salicylic acid. Once the reaction is complete, the student collects 1.22 gg of aspirin.    Determine the percent yield of aspirin for the reaction. Express your answer using three significant figures.

3 Consider the reaction 1205(g) + 5 CO(g) →→ 5CO2(g) + ¹2(g) 80.0 grams of iodine pentoxide, 1205 (molar mass = 333.80g/mol), reacts with 38.0 grams of carbon monoxide (molar mass 28.01g/mol). Determine the mass of iodine that could be produced. Place only the numeric answer in the box, no units/% sign. If the answer is 12.34g O2, only type 12.34 in the box. Round all answers to 2 decimal places N