SiCl4 + O2 SIO2 + Cl2The table shows an experimental record for the above reaction.Experimental RecordTrial Starting Amount of SICI4 Starting Amount of O2 Actual Yield of SiO2100 g32.96 g100 g50 g25.2 g75 ga. Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work.b. Based on the percentage yield in Trial 2. explain what ratio of reactants is more efficient for the given reaction.

Given reaction, SiCl4 + O2 -> SiO2 + Cl2. Molar mass of SiCl4 = 170gMolar mass of O2 = 32g. Trial…

SiCI4 + O2- SiO2 + Cl2 The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SICI4 Starting Amount of 02 Actual Yield of SiO2 100 g 100 g 32.96 g 75 g 50 g 25.2 g 2

SiCI4 + O2- SiO2 + Cl2 The table shows an experimental record for the above reaction. Experimental Record Trial Starting Amount of SICI4 Starting Amount of 02 Actual Yield of SiO2 100 g 100 g 32.96 g 75 g 50 g 25.2 g 2

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...

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Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

SiCl4 + O2 SIO2 + Cl2
The table shows an experimental record for the above reaction.
Experimental Record
Trial Starting Amount of SICI4 Starting Amount of O2 Actual Yield of SiO2
100 g
32.96 g
100 g
50 g
25.2 g
75 g
a. Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work.
b. Based on the percentage yield in Trial 2. explain what ratio of reactants is more efficient for the given reaction.

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