In the following reaction, oxygen is the excess reactant. SiCl4 + O2 → SiO2 + Cl2

The table shows an experimental record for the above reaction.

Experimental Record
Trial Starting Amount of SiCl4 Starting Amount of O2 Actual Yield of SiO2
1 100 g 100 g 32.96 g
2 75 g 50 g 25.2 g

Calculate the percentage yield for SiO2 for Trial 1. Also, determine the leftover reactant for the trial. Show your work.
Based on the percentage yield in Trial 2, explain what ratio of reactants is more efficient for the given reaction.

i think that the answer is c

5.6⋅10−^19  j

do you need the explaination?

the seeing the electronic configuration we can say that the element is fluorine.

fluorine is the most electronegative element in the periodic table.

but by only seeing the configuration we cannot say about its reactivity because we don't know if its configuration after excitation or by addition of electrons.

but if not then, it is the lightest halogen and exists as a highly toxic pale yellow diatomic gas at standard conditions. as the most electronegative element, it is extremely reactive: almost all other elements, including some noble gases, form compounds with fluorine.