### Preparation of Silicon Tetrachloride (SiCl₄) by Heating Silicon in Chlorine GasThe reaction for forming Silicon Tetrachloride involves silicon (Si) and chlorine gas (Cl₂) as follows:\[ \text{2Cl}_2(\text{g}) + \text{Si}(\text{s}) \rightarrow \text{SiCl}_4(\text{l}) \]This educational module explores the stoichiometry of this reaction with the following tasks:1. **Calculate the Number of Moles of Cl₂ Required:** - Given: Formation of 0.268 moles of SiCl₄. - Assume an excess of Si is present. - Calculate the moles of Cl₂ needed for this reaction.2. **Determine the Moles of Silicon Required:** - Find the moles of Si necessary to produce the given amount of SiCl₄.**Instructions:**- To calculate the moles of Cl₂: Utilize the molar ratio from the balanced chemical equation.- Determine the moles of Si based on the ratio from the equation.This practical example provides insights into chemical reaction calculations and stoichiometric principles.

Answered: Image /qna-images/answer/1aae4766-b754-4101-82d7-d91d7bcb8158.jpg

Silicon tetrachloride (SiCl4) can be prepared by heating Si in chlorine gas: 2C12(g) + Si(s) SiCl4(0) Calculate the number of moles of Cl2 required to form 0.268 moles of SiCI4. Assume excess Si. moles Cl2 -> Determine the moles of silicon required to form the amount of SiCl4 given above. moles Si

Silicon tetrachloride (SiCl4) can be prepared by heating Si in chlorine gas: 2C12(g) + Si(s) SiCl4(0) Calculate the number of moles of Cl2 required to form 0.268 moles of SiCI4. Assume excess Si. moles Cl2 -> Determine the moles of silicon required to form the amount of SiCl4 given above. moles Si

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.83QE: Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and...

See similar textbooks

Similar questions

Silicon forms a series of compounds analogous to the al-kanes and having the general formula SinH2n+2. The first of these compounds is silane, SiH4, which is used in the electronics industry to produce thin ultrapure silicon films. SiH4(g) is somewhat difficult to work with because it is py-ropboric at room temperature—meaning that it bursts into flame spontaneously when exposed to air. (a) Write an equation for the combustion of SiH4(g). (The reaction is analogous to hydrocarbon combustion, and SiO2 is a solid under standard conditions. Assume the water produced will be a gas.) (b) Use the data from Appendix E to calculate ? for this reaction. (c) Calculate G and show that the reaction is spontaneous at 25°C. (d) Compare G for this reaction to the combustion of methane. (See the previous problem.) Are the reactions in these two exercises enthalpy or entropy driven? Explain.
Calcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) Is the reaction endothermic or exothermic?
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.
Calculate the maximum mass of pure iron that can be produced by the concentration of 350 t of coke. Please don't round when doing math
As of 2018, -95% of hydrogen is produced from fossil fuels. One of the most important reactions of this type is the steam reforming of methane (CHA). Write a balanced chemical equation based on the following description: gaseous methane reacts with steam to form carbon monoxide and hydrogen gases. 3c, 2- Reset 1 3 4 7 9 -> (s) (1) (g) (aq) H. Но СНО Не Co x H20 00 LO
Given the data in the table below, AHrxn for the reaction Ca(OH); + 2H;AsO4 → Ca(H;AsO4)2 + 2H;O is _ kJ. [A] -4219 (B] -130.4 [C] -4519 [D] -76.4 AH, (kJ/mol) -986.6|| Substance Ca(ОН), HASO, Ca(H;AsOa)2 -900.4 -2346.0 H;0 -285.9 O A В C D
Give correct detailed Solution
When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s) + CO₂(g) What is the mass of calcium carbonate needed to produce 35.0 L of carbon dioxide at STP? Express your answer with the appropriate units. View Available Hint(s) mass of CaCO3 Submit = Part B 0 370.8 HÅ atm Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining ? Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10 (9) + 1302 (g)→8CO2 (g) + 10H₂O (1) At 1.00 atm and 23 °C, what is the volume of carbon dioxide formed by the combustion of 2.20 g of butane? Express your answer with the appropriate units.
Ethylene (C2H4) plays an important role in the ripening of certain fruits and vegetables. It is sometimes supplemented under controlled conditions at produce—processing facilities but is also produced naturally by many fruit-bearing plants. Although the actual process by which plants produce ethylene is a complex one, imagine that it is produced by the simple breakdown of glucose according to the equation: C6H12O6(s)⟶3C2H4(g)+3O2(g) Given S°= 212.1 J/molK, ΔG°= -910.56 kJ/mol and ΔH°= -1274.5 kJ/mol for C6H12O6 (s). Using the tabulated ΔG° values in the appendix, calculate ΔG° for the reaction in kJ/mol. Please include 5 significant figures in your answer and do not include units.
Please don't provide handwritten solution .....
Consider the reaction below. The reaction quotient for a specific moment is 3.42-10³. If the equilibrium constant is 1.16. 104, what needs to happen in order for the reaction to reach equilibria? Select all that apply. 2 A+ 4 B5 C There will be a net gain in reactant. There will be a net gain in product. The forward reaction will procede more than the reverse reaction. The reverse reaction will occur more than the forward reaction. The system will shift to the left. The system will shift to the right.