If steel wool (iron) is heated until it glows and is placed in a bottle containing pureoxygen, the iron reacts spectacularly to produce iron(III) oxide.msp;1.25 g of iron is heated and placed in a bottle containing 0.0204 mole of oxygen gas,what mass of iron(III) oxide is produced?

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.

If you have 35.67g of Copper (II) Sulfate how many grams of just copper are present? Convert 35.67g of Copper (II) Sulfate into mols . Convert 35.67g of Copper (II) Sulfate into molecules of Copper (II) Sulfate.

The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 X

Consider the following reactions:CoO (s) + CO (g) D CO2 (g) + Co (s) Kc(1) = 490.2 CoO (s) + 2 H2 (g) D 2 Co (s) + 2 H2O (g) Kc(2) = 4.5 x 103a. Write the overall equation for the reaction of hydrogen gas and carbon dioxide gas to produce carbon monoxide gas and steam.

Using the initial mass 1.510 g and the molecular formula of the hydrate CuCl2​⋅2H2​O). Predict the expected mass of water that should be released if heated.

A student prepares phosphorous acid by reacting solid phosphorous triiodide with waterPI₃(s) + 3 H₂O(l) → H₃PO₃(s) + 3 HI(g)The student needs to obtain 0.359 L of phosphorous acid (d=1.651g/mL). The procedure calls for a 43.3 % excess of water and a yield of 70.8%. How much phosphorous triiodide should be weighed out?

Ammonia (NH3) is an important compountd is used in large amounts for the manufacture of nitrogenous fertilizers, nylon and many other important compounds. It is manufactured by the catalytic reaction between nitrogen between nitrogen and hydrogen, according to the following equation; N2(g) +H2(g) = NH;(g) When 1.20 mol nitrogen and 1.20 mol hydrogen are mixed together in a closed vessel, 30% of the nitrogen is converted into ammonia. a. Calculate the moles of nitrogen gas that will be present in the vessel? (only 3 decimal places) mol b. Calculate the moles of hydrogen gas that will be present in the vessel? (only 3 decimal places) mol c. Calculate the moles of ammonia gas that will be present in the vessel? (only 3 decimal places) Activate W mol d. What is the number of moles of nitrogen gas that has reacted? (only 3 decimal places) 10:09 Links 18°C 1O 23-Nov-21

A 2.69 gram sample of a KCl and KClO3 mixture was found to contain 0.01268 mol of KClO3. What is the percent by mass of KClO3 in the original mixture? Report your answer with three significant figures.

A reaction is performed where 10.0 g K2S(s) are added to 250.0 mL of a 0.855 M HCl (aq) solution. Write a balanced equation for the reaction that would occur. Calculate the maximum number of moles of the gaseous product that can form? Which substance is the limiting reactant? How many moles of the non-limiting (or excess) reactant remain if the reaction goes to completion?What is the volume of the gas that forms if it is collected at 0.987 atm and 27.5°C?