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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

4. Calculate the percent yield for the reaction below if 75.0 g of phosphorous reacts with 345 g of chlorine to produce 111.0 g of phosphorous trichloride. P:(s) + 6 Cl,(g) –→ 4 PCI3(1)
The combustion of propane occurs through the following chemical reaction. C3 H3 (g) + 5 O2 (g). - 3 CO2 (g) + 4 H,O (g) -> How many grams of H20 can be made by reacting 11.27 grams of oxygen gas?
Nitric oxide (NO) reacts with oxygen gas to form nitrogen dioxide (NO2), a dark-brown gas: 2NO(g) + O (g) ⟶ 2NO (g) In one experiment 0.886 mole of NO is mixed with 0.503 mole of O2. Calculate which of the two reactants is the limiting reactant. Calculate also the number of moles of NO2 produced.
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?
Fill in the blanks using the other image.
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