When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose some calcium carbonate is sealed into a limekiln of volume 550. L and heated to 520.0 °C. When the amount of CaCO3 has stopped changing, it is found that 8.46 kg have disappeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 520.0 °C. Round your answer to 2 significant digits. P Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value. K₁ = 0 X 3

Because carbon and silicon are both elements in group 14 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but in some cases, carbon and silicon compounds that seem to have analogous structures have very different chemical characteristics. For example, carbon tetrachloride, CCl4, is very stable in the presence of water, but silicon tetrachloride, SiCl4, reacts quickly with water. The unbalanced equation for this reaction is SiCl4 + H2O → Si(OH)4 + HCl Balance this equation. Write a conversion factor that could be used to convert between moles of SiCl4 and moles of H2O. How many moles of SiCl4 react with 24 moles of water? Write a conversion factor that could be used to convert between moles of Si(OH)4 and moles of water. How many moles of Si(OH)4 form when 4.01 moles of H2O react with an excess of SiCl4?

Upon heating 134 g MgSO4 · 7 H2O:(a) how many grams of water can be obtained? (b) how many grams of anhydrous compound can be obtained?

What is the CORRECT equilibrium constant expression for the reaction of N2O (g) and O2(g) to produce NO(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.

The extraction of aluminum metal from the aluminum hydroxide in bauxite ore by the Hall-Héroult process is one of the most remarkable success stories of late 19th century practical chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina and water: 2 Al(OH)3(s)-Al₂O3(s) + 3 H₂O(g) In the second step, alumina and carbon react to form aluminum and carbon dioxide: 2 Al₂O3(s)+3 C(s)-4 Al(s) + 3 CO₂(g) Write the net chemical equation for the production of aluminum from aluminum hydroxide and carbon. Be sure your equation is balanced. Explanation Check 80 E5 ローロ X On F6 S MacBook Air F7 DII FB FO A Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Access F10 A F11 ola Ar 00

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Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

Consider the reaction: N2(g) + 3H2(g) 2NH3(g) where Kc = 0.500 at 400 °C. If 50.0 L reaction vessel contains 1.000 mole N₂; 3.000 mole H₂ and 0.050 mole NH3, which of the following is TRUE? The reaction based on the following parameters is in equilibrium. More ammonia will be produced as the reaction approaches equilibrium. Data provided is not enough to warrant a conclusion regarding equilibrium. More ammonia will dissociate as the reaction approaches equilibrium.

A 1.00-L flask was filled with 2.14 mol gaseous SO2 and 2.14 mol gaseous NO2 and heated. After equilibrium was reached, it was found that 1.55 mol gaseous NO was present. Assume that the reaction SO2 (g) + NO, (g) = SO3(g) + NO(g) occurs under these conditions. Calculate the value of the equilibrium constant, K, for this reaction. HOW DO WE GET THERE? What are the equilibrium concentrations of SO2, NO2, and SO3? [SO2] = [NO2] = M [SO3] = M