When an identical 4.008 g of sulfur is burned completely in a restricted amount of air, it again combines with oxygen to form a single gaseous product, but this time the total mass of the product is 8.008 g. What is the mass perfect of sulfur and oxyegn in the gaseous product?

4.84. Aluminum chloride (AICI3) is used as a catalyst in the production of polyisobutylene, which is used in automobile tires. Scrap aluminum metal reacts with chlorine gas (Cl,2) to produce AICI; . Suppose that 2.70 g of Al and 7.10 g of Cl2 are mixed. What is the maximum mass of AlCl, that could be formed?

A student synthesizes tin oxide to create a compound with generic formula SnxOy. She does this by combining 30.80 g of tin and when the tin oxide product is produced, the total mass of the product is 39.10 g. Given that oxygen has a molar mass 15.999 g⋅mole-1, the number of moles of oxygen in the product is A) 0.51888 B) 132.81

According to the following reaction, how many grams of mercury will be formed upon the complete reaction of 31.3 grams of mercury(II) oxide? 2HgO(s) → 2Hg(l) + O₂(g) ||| g mercury

If 5.3 g of hydrogen gas is reacted with 12.6 g of oxygen gas to produce water, the hydrogen is the A reagent and the oxygen is the A reagent.

Write balanced chemical eauations for the following reactions. The reaction of aqueous iron(III) nitrate and aqueous potassium carbonate to produce aqueous potassium nitrate and solid iron(II) carbonate.

Chemical Bonding -.. V Pennsylvania Acces... Department of Hu.. Bvlgari Man In Blac.. O CHEMICAL REACTIONS Identifying the limiting reactant in a drawing of a mixture The drawing below shows a mixture of molecules: key carbon hydrogen nitrogen sulfur oxygen chlorine Suppose the following chemical reaction can take place in this mixture: 2C,H,(g)+50,(g) → 4 CO,(g)+2H,O(g) Of which reactant are there the most initial moles? Enter its chemical formula: Of which reactant are there the least initial moles? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula: Explanation Check

Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the reaction of an acid on an alkaline earth metal peroxide, such as barium peroxide. BaO2 + HCl ---> H2O2 + BaCl2 What amount of hydrogen peroxide should result when 1.17 g of barium peroxide is treated with 28.0 mL of hydrochloric acid solution containing 0.0288 g of HCl per mL? _____ g H2O2

(b) An unknown mass of Na3PO4(s) is dissolved in water to form 50.00 mL of solution. This is Solution A. Then 10.00 mL of Solution A is diluted with water to 50.00 mL. The final solution is Solution B. 20.00 mL of Solution B contains 4.408 x 1020 sodium ions. (NA = 6.022 x 1023 mol-1) Calculate the mass of Na3PO4(s) that was dissolved to form Solution A.

An impure sample of table salt (NaCl) that was dissolved in water and treated with silver nitrate to form silver chloride. If the initial sample had a mass of 1.741 g and the final mass of the AgCl was found to be 4.084 g, what is the mass percent of NaCl in the impure sample?