HF + SIO₂ → H₂SiF + H₂O Write the balanced reaction in the space below. balanced reaction: How much H₂SiF can be produced from 3.00 moles of HF? moles of H₂SiF6: If 3.00 moles of HF and 1.50 moles of SiO, were initially present, what is the fractional excess of SiO,?
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
The following reaction is unbalanced.
![**Question:**
What is the percent excess of SiO₂?
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**Input Field:**
percent excess of SiO₂: [Text Box] %
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**Description:**
This image presents a question asking for the calculation of the percent excess of Silicon Dioxide (SiO₂). It includes an input field where the user is expected to enter their answer. The input field is followed by a percentage symbol. There are no graphs or diagrams included in this image.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F135d4a40-2572-4c62-8b31-300ca8461b64%2Fad2d104d-b597-4a32-8bd7-7e146469bfe8%2F0m0dxau_processed.png&w=3840&q=75)
![**Chemical Reaction and Stoichiometry Problem**
**Reaction:**
\[ \text{HF} + \text{SiO}_2 \longrightarrow \text{H}_2\text{SiF}_6 + \text{H}_2\text{O} \]
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1. **Write the balanced reaction in the space below.**
**Balanced reaction:**
\[ \underline{\hspace{10cm}} \]
2. **How much \(\text{H}_2\text{SiF}_6\) can be produced from 3.00 moles of HF?**
**Moles of \(\text{H}_2\text{SiF}_6\):**
\[ \underline{\hspace{10cm}} \]
3. **If 3.00 moles of HF and 1.50 moles of \(\text{SiO}_2\) were initially present, what is the fractional excess of \(\text{SiO}_2\)?**
\[\underline{\hspace{10cm}} \]
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This exercise involves balancing a chemical equation and calculating the stoichiometry of the reaction products and reactants. Students are tasked with determining the balanced form of the reaction, the amount of a specific product formed, and identifying the limiting and excess reagents to calculate the fractional excess of one of the reactants.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F135d4a40-2572-4c62-8b31-300ca8461b64%2Fad2d104d-b597-4a32-8bd7-7e146469bfe8%2Fgsogixv_processed.png&w=3840&q=75)
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