Question 4 of 37 Submit Write a balanced chemical equation based on the following description: propanol, C̟H,OH(I) burns in air to produce gaseous carbon dioxide and water vapor 04- O3. 02 02+ 03+ 04+ 1 4 6. 7 9 O2 O3 04 (s) (1) (g) (aq) Cr Са H. Pr Cb P. +

Write a balanced chemical equation based on the following description: solid sodium reacts with chlorine gas to produce solid sodium chloride. Na(s)+Cl2(g)_

Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the O-0 decomposition of solid calcium carbonate (CaCO3) into solid calcium oxide and gaseous carbon dioxide. x10 Ar 2. Suppose 86.0L of carbon dioxide gas are produced by this reaction, at a temperature of 230.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Be sure your answer has the correct number of significant digits.

Dry ice is solid carbon dioxide. Instead of melting, solid carbondioxide sublimes according to the equation:CO2(s) ------------>CO2(g) When dry ice is added to warm water, heat from the water causesthe dry ice to sublime more quickly. The evaporating carbon dioxide produces a dense fog often used to create special effects. In a simple dry ice fog machine, dry ice is added to warm water in a Styrofoam cooler. The dryice produces fog until it evaporates away, or until the water gets too cold to sublime the dry ice quickly enough. A small Styrofoam cooler holds15.0 L of water heated to 85°C. Use standard enthalpies of formation to calculate the change in enthalpy for dry ice sublimation, and calculate themass of dry ice that should be added to the water so that the dry ice completely sublimes away when the water reaches 25 °C. Assume no heat loss to the surroundings. (The ∆H°f for CO2(s) is -427.4 kJ/mol.)

The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. 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 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 0.50 kg of potassium chlorate:

||| O Microsoft O The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) 2MnO₂ (s) + 2 CO₂(g) W O CHEMICAL REACTIONS Reaction sequence stoichiometry In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s)→ 3Mn(s) + 2 Al₂O₂ (s) Microsoft esc Suppose the yield of the first step is 73.% and the yield of the second step is 86.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. G Microsoft 6.52.210... Explanation B ! Check 9,270 280 103 x10 HE X OCT 24 ロ・ロ Ś III E % LC ustv ♫ 6 2 & 7 9 © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DZA 8 9 1/5 W 0 30 Simrat V + 11 ? olo Ar 2…

MTBE (C5H12O) is a high-octane gasoline additive with a sweet, nauseating odor. Because small amounts of MTBE have contaminated the drinking water in some towns, it is now banned as a fuel additive in many areas. MTBE reacts with O2 to form CO2 and H2O. Write a balanced equation for the combustion of MTBE. Do not included states of matter in your answer.

Combustion of hydrocarbons such as hexane (C6H₁4) produces carbon dioxide, a "greenhouse gas." Greenhouse gases in the Earth's atmosphere can trap the Sun's heat, raising the average temperature of the Earth. For this reason there has been a great deal of international discussion about whether to regulate the production of carbon dioxide. 1. Write a balanced chemical equation, including physical state symbols, for the combustion of liquid hexane into gaseous carbon dioxide and gaseous water. 2. Suppose 0.220 kg of hexane are burned in air at a pressure of exactly 1 atm and a temperature of 17.0 °C. Calculate the volume of carbon dioxide gas that is produced. Round your answer to 3 significant digits. ローロ X 0 x10

Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N,(9)+3 H,(g)→2NH,(g) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g)+20,(9)→HNO;(g)+H,0(g) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.

$ P O CHEMICAL REACTIONS Reaction sequence stoichiometry There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide (CaC₂) and water react to form acetylene (C₂H₂) and calcium hydroxide: C₂H₂(g) + Ca(OH)₂ (s) In the second step, acetylene (C₂H₂), carbon dioxide and water react to form acrylic acid (CH₂CHCO₂H): 6C₂H₂ (g) + 3C0₂(g) + 4H₂O(g) 5 CH₂CHCO₂H (g) - CaC₂ (s) + 2H₂O(g) → C₂H₂(g) Suppose the yield of the first step is 87.% and the yield of the second step is 91.%. Calculate the mass of calcium carbide required to make 8.0 kg of acrylic acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation % 5 T B Check 20 A 6 Y H N 0.0 0° ロ・ロ 믐 20 MacBook Pro & X 7 U 3 * 8 M I K ( 9 H V. O L ) O P A. T © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility || O { [ ? + 11 = I 0/3 11 Q 1 Leah delete 0 G…