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A Consider the following reaction: SICI4+ 4H2₂0 → H₂SiO + 4HCI When molecules of SiCI and H₂O were allowed to react, 61.0 molecules of H SIO and some molecules of HCI were 4 '4' formed. There was no excess or leftover reactant. How many molecules of HCI were formed? 244 molecules 83.0 molecules 72.0 molecules 432 molecules

A Consider the following reaction: SICI4+ 4H2₂0 → H₂SiO + 4HCI When molecules of SiCI and H₂O were allowed to react, 61.0 molecules of H SIO and some molecules of HCI were 4 '4' formed. There was no excess or leftover reactant. How many molecules of HCI were formed? 244 molecules 83.0 molecules 72.0 molecules 432 molecules

Chemistry
Chemistry
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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
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**Chemical Reaction Analysis:** Consider the following reaction: \[ \text{SiCl}_4 + 4\text{H}_2\text{O} \rightarrow \text{H}_4\text{SiO}_4 + 4\text{HCl} \] When molecules of \(\text{SiCl}_4\) and \(\text{H}_2\text{O}\) were allowed to react, 61.0 molecules of \(\text{H}_4\text{SiO}_4\) and some molecules of \(\text{HCl}\) were formed. There was no excess or leftover reactant. How many molecules of \(\text{HCl}\) were formed? **Answer Options:** - 244 molecules - 83.0 molecules - 72.0 molecules - 432 molecules **Selected Answer:** 72.0 molecules **Explanation:** According to the balanced chemical equation, one molecule of \(\text{SiCl}_4\) reacts with four molecules of \(\text{H}_2\text{O}\) to produce one molecule of \(\text{H}_4\text{SiO}_4\) and four molecules of \(\text{HCl}\). Since 61.0 molecules of \(\text{H}_4\text{SiO}_4\) are formed, the same number of complete reactions (61.0) occurs, resulting in: \[ 61.0 \, \text{reactions} \times 4 \, \text{molecules of HCl per reaction} = 244 \, \text{molecules of HCl} \] The final choice (72.0 molecules) was marked, which may not align with the stoichiometry given the information provided.
Transcribed Image Text:**Chemical Reaction Analysis:** Consider the following reaction: \[ \text{SiCl}_4 + 4\text{H}_2\text{O} \rightarrow \text{H}_4\text{SiO}_4 + 4\text{HCl} \] When molecules of \(\text{SiCl}_4\) and \(\text{H}_2\text{O}\) were allowed to react, 61.0 molecules of \(\text{H}_4\text{SiO}_4\) and some molecules of \(\text{HCl}\) were formed. There was no excess or leftover reactant. How many molecules of \(\text{HCl}\) were formed? **Answer Options:** - 244 molecules - 83.0 molecules - 72.0 molecules - 432 molecules **Selected Answer:** 72.0 molecules **Explanation:** According to the balanced chemical equation, one molecule of \(\text{SiCl}_4\) reacts with four molecules of \(\text{H}_2\text{O}\) to produce one molecule of \(\text{H}_4\text{SiO}_4\) and four molecules of \(\text{HCl}\). Since 61.0 molecules of \(\text{H}_4\text{SiO}_4\) are formed, the same number of complete reactions (61.0) occurs, resulting in: \[ 61.0 \, \text{reactions} \times 4 \, \text{molecules of HCl per reaction} = 244 \, \text{molecules of HCl} \] The final choice (72.0 molecules) was marked, which may not align with the stoichiometry given the information provided.
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