Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treatingmolten sulfur with gaseous chlorine:S8(l) + 4 Cl2(g) → 4 S2Cl3(l)Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2,(a) Which is the limiting reactant?(b) What is the theoretical yield of S2Cl2?(c) What mass of the excess reactant remains when the reaction is completed

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.

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?

A website promoting the use of alternative energy vehicles and hybrid technologies claims that "A typical automobile in the USA uses about 500 gal of gasoline every year, producing about 5 tons of carbon dioxide." To determine the truth of this statement, calculate how many tons of carbon dioxide are produced when 500.0 gal of gasoline are combusted. Assume that the primary ingredient in gasoline is octane, C H₁ (1), which has a density of 0.703 g · mL-¹. 18 CO₂ produced: tons

The theoretical yield of a reaction is the amount of product obtained if the limiting reactant is completely converted to product. Consider the reaction: N₂(g) + O₂(g) → 2 NO(g) If 5.220 g N₂ is mixed with 9.660 g O₂, calculate the theoretical yield (g) of NO produced by the reaction. g

The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2 (g) + 3H2 (g) → 2 NH, (g) a What is the maximum mass of ammonia that can be produced from a mixture of 1.00 x 10° g N2 and 5.60 x 102 g H2? Mass = g

Consider the following balanced equation for the combustion of butane, a fuel often used in lighters.2 C4H10(g) + 13 O2(g) → 8 CO2(g) + 10 H2O(g)Complete the following table, showing the appropriate masses of reactants and products. If the mass of a reactant is provided, fill in the mass of other reactants required to completely react with the given mass, as well as the mass of each product formed. If the mass of a product is provided, fill in the required masses of each reactant to make that amount of product, as well as the mass of the other product that is formed.   Mass C4H10 Mass O2 Mass CO2 Mass H2O _____ 2.11 g _____ _____ 5.32 g _____ _____ _____ _____ _____ 13.12 g _____ _____ _____ _____ 8.44 g 252 mg _____ _____ _____ _____ _____ 198 mg _____

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + Mn0,(s) - MnCl, (aq) + 2 H,O(1) + Cl, (g) A sample of 41.7 g MnO, is added to a solution containing 49.7 g HCI. What is the limiting reactant? HCI O MnO2 What is the theoretical yield of Cl, ? theoretical yield: g Cl2 If the yield of the reaction is 84.3%, what is the actual yield of chlorine? actual yield: g Cl,

For the following reaction, 15.5 grams of phosphorus (P4) are allowed to react with 41.6 grams of chlorine gas. phosphorus (P4)(s) + chlorine(g) → phosphorus trichloride (1) What is the maximum mass of phosphorus trichloride that can be formed? Mass= g What is the FORMULA for the limiting reactant? What mass of the excess reagent remains after the reaction is complete? Mass= g