Titanium reacts with iodine to form titanium(III) iodide, emitting heat, via the following reaction: 2Ti(s)+3I2(g)→2TiI3(s), ΔHrxn=−839kJ Determine the mass of titanium that reacts if 1.53×103 kJ of heat is emitted by the reaction. Express your answer to three significant figures and include the appropriate units.   Determine the mass of iodine that reacts if 1.53×103 kJ of heat is emitted by the reaction.   Express your answer to three significant figures and include the appropriate units.

Commercial drain cleaners contain sodium hydroxide and aluminum. When water is added to this mixture, the heat that is generated will melt grease and the gas that is created will stir up the particles that are clogging the drain. If the process proceeds according to the following reaction: 2 Al (s) + 2 NaOH (aq) + 6 H2O (l) → 2 NaAl(OH)­4 (aq) + 3 H2 (g)   If you use 5.6 g of Al (s) and excess sodium hydroxide, how many liters of H2 (g) at 742 mm Hg and 22.0 ˚C are produced?

Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N,(0) + 3 H,(9) → 2 NH,(9) ΔΗ-92. k In the second step, ammonia and oxygen react to form nitric acid and water: NH,(9) + 20,(9) → HNO3(g) + H,O(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. ?

The manufacture of nitrogen trifluoride is a growing industry, due to its use as a plasma etchant in the semiconductor industry. Nitrogen trifluoride can be synthesized by passing a current through a high-temperature mixture of ammonium fluoride and hydrogen fluoride, with hydrogen gas as a byproduct. In one synthesis, 1.20x10^3g ammonium fluoride is reacted with1.20x10^3g hydrogen fluoride to produce 5.00x10^2g nitrogen trifluoride. What is the limiting reactant, excess reactant, theoretical yield of nitrogen trifluoride, percent yield, and mass of excess reactant remaining after the reaction?

One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CUSO 4(aq) Cu(s) + FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 450. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 147. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 3 significant digits. ?

When aqueous solutions of magnesium chloride (MgCl2) and silver nitrate (AgNO3) are mixed, the products are solid silver chloride and aqueous magnesium nitrate. Write the balanced chemical equation for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.)

Ethanol, C,H,O, is most often blended with gasoline - usually as a 10 percent mix - to create a fuel called gasohol. Ethanol is a renewable resource and ethanol-blended fuels, like gasohol, appear to burn more efficiently in combustion engines. The heat of combustion of ethanol is 326.7 kcal/mol. The heat of combustion of 2-methylheptane, C3H18, is 1.306×10³ kcal/mol. How much energy is released during the complete combustion of 482 grams of 2-methylheptane ? kcal Assuming the same efficiency, would 482 grams of ethanol provide more, less, or the same amount of energy as 482 grams of 2- methylheptane v more less the same amount

Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (MgSO₄･7H₂O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 57.75 g. How many grams of the original salt mixture must you add to 1.000 L of water to make a 0.100 M solution of Mg²⁺ ion?

What is the sum of coefficients from the following reaction (both products and reactants)? X.3H2O + Heat ---> X can be any element.

Consider the reaction. heat 2 Al(s) + Fe,0,(s) Al, 0,(s) + 2 Fe(1) If 10.7 kg Al reacts with an excess of Fe, O3, how many kilograms of Al,O, will be produced? mass of Al, O, produced: kg * TOOLS x10