Disulfur dichloride, S₂Cl₂, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine: Sg(t) + 4 Cl₂(g) 4 S₂Cl₂() A Starting with a mixture of 84.7 g of sulfur and 18.0 g of Cl₂, A. Which is the limiting reactant? O sulfur O chlorine disulfur dichloride B. What is the theoretical yield of S₂Cl₂? gS₂Cl₂ C. What mass of the excess reactant remains when the reaction is completed? g excess reactant

Elemental silicon can be produced by the reduction of silicon dioxide, or sand, with carbon: SiO2 + 2 C ¡ Si + 2 CO When 35.0 kg of SiO2 reacts with 25.3 kg of carbon, and 14.4 kg of silicon is recovered, what is the percent yield for the reaction?

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A compound is composed of the elements, carbon, hydrogen, and oxygen only. Combustion of the compound produces CO2 and H2OC?H?O? + O2 ➝ CO2 + H2OCombustion of a 10.000 g sample of the compound produces the products shown in the table below. Product Mass (grams) CO2 22.837 H2O 5.843             Determine the empirical formula for the compound. [If an element has a subscript of 1, enter 1]Empirical Formula: CAnswerHAnswerOAnswer

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

When propane (C3Hg) reacts with oxygen, carbon dioxide and water are produced. The balanced equation for this reaction is C3 Hs (g) + 502 (g) → 3CO2(g) + 4H2O(g) If 10 moles of oxygen react, The reaction consumes moles of propane (C3H8). The reaction produces moles of carbon dioxide and moles of water.

When sulfuric acid reacts with calcium hydroxide, calcium sulfate andwater are produced. The balanced equation for this reaction is: H2S04(aq) + Ca(OH)2(s) CaSO4(s) + 2H2O(l) If 2 moles of calcium hydroxide react, The reaction consumes  moles of sulfuric acid.   The reaction produces moles of calcium sulfate and   moles of water.

A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, CgH5Br, and HBr. C6H6 + Br2 --> C6H5Br + HBr What is the theoretical yield of bromobenzene in this reaction when 29.2 g of benzene reacts with 70.5 g of bromine? grams Which chemical is the limiting reactant? Select an answer If the actual yield of bromobenzene was 39.5 g, what was the percent yield?

Combustion of methane is an important fuel source. The combustion produces CO2 and H2O. What is the percent atom economy for the production of H2O in the reaction below?CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g)

For the following reaction, 15.9 grams of glucose (C6H1206) are allowed to react with 12.4 grams of oxygen gas > carbon dioxide(g) + water( glucose (CH1206(s) + oxygen(g) What is the maximum amount of carbon dioxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams