When limestone, which is principally CaCO3, is heated, car- bon dioxide and quicklime, CaO, are produced by the reaction CaCO3(s) CaO(s) + CO₂(g). If 17.5 g of CO₂ is produced from the thermal decomposition of 42.73 g of CaCO3, what is the percentage yield of the reaction?

Chloramine is a toxic gas that can form in swimming pools by the reaction of hypochlorous acid, used to sanitize pool water, with ammonia, a component of sweat and urine. Chloramine gas, NH₂Cl(g), is the cause of the identifiable 'pool smell'. The balanced chemical equation for the reaction of hypochlorous acid and ammonia is: HOCl(aq) + NH₃(aq) → NH₂Cl(g) + H₂O(l) A swimming pool holding 9.50 × 10⁴ gallons of water. 1.00 gallons HOCl sanitizer is enough to sanitize 1.00 × 10⁴ gallons of pool water. The sanitizer has a concentration of 12.00 mg/L of Cl atoms. Determine the moles of chloramine are produced if ammonia is in excess. (1 gal = 3.785 L)

Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, from the complete reaction of 15.6 grams H, in the presence of excess N, gas according to the following balanced chemical equation: N,(g) + 3 H,(g) → 2 NH,(g)

Chlorine gas can be produced in the laboratory by adding concentrated hydrochloric acid, HCl, to manganese(IV) oxide according to the following reaction: MnO2 (s)   +   4 HCl (aq)   →   MnCl2 (aq)   +   2 H2O (l)   +   Cl2 (g) What mass of MnO2 is required to produce 48.4 g Cl2 by the following reaction? Be sure to enter a unit with your answer.

In a reaction to produce NaF, 3.50 g of HF and 1.26 of Na2SiO3 are reacted according to the following: Na2SiO3 (s) + HF (aq) →H2SiF6 (aq) + NaF (aq) + H2O (l) (a) Balance the equation.   (b) Calculate the theoretical yield of NaF.   (c) If 0.792 g of NaF is formed, calculate the percent yield.

Methanol can be produced through the reaction of CO and H, in the presence of a catalyst. catalyst CO(g) + 2H,(g) - CH̟OH() If 75.0 g of CO react to produce 68.4 g CH,OH, what is the percentage yield of CH,OH?

Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 5O2(g) -> 2P2O5(g)   In the second step, diphosphorus pentoxide and water react to form phosphoric acid H3PO4: P2O5(g) + 3H2O(l) -> 2H3PO4(l)   Suppose the yield of the first step is 69.% and the yield of the second step is 82.%. Calculate the mass of phosphorus required to make  1.0kg of phosphoric acid. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

When butane (C,H10) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is: 2C, H10 (8) + 1302 (g) → 8CO2(g) + 10H; O(g) If 39 moles of oxygen react, The reaction consumes |moles of butane (C,H10). moles of carbon dioxide and |moles of water. The reaction produces

A sample of calcium metal with a mass of 2.00 was reacted with excess oxygen. The following equation represents the reaction that took place: 2Ca(s)+O2(g)-> 2CaO(s) the isolated product CaO weighed 2.26g. What was the percent yield of the reaction?

Q 3 Hydrogen cyanide, HCN, is prepared from ammonia, air, and natural gas (CH4) by the following process: Pt 2NH3(g) + 302(8) + 2CH4(g) 2HCN(g) + 6H20(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 11.5 g NH3, 12.0 g 02, and 10.5 g CH4, what is the maximum mass in grams of hydrogen cyanide that could be made, assuming the reaction goes to completion as written?