A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr. C6H6 + Br2 --> C6H5B + HBr What is the theoretical yield of bromobenzene in this reaction when 39.3 g of benzene reacts with 61.8 g of bromine? grams Which chemical is the limiting reactant? Select an answer If the actual yield of bromobenzene was 31.7 g, what was the percent yield?
Electronic Effects
The effect of electrons that are located in the chemical bonds within the atoms of the molecule is termed an electronic effect. The electronic effect is also explained as the effect through which the reactivity of the compound in one portion is controlled by the electron repulsion or attraction producing in another portion of the molecule.
Drawing Resonance Forms
In organic chemistry, resonance may be a mental exercise that illustrates the delocalization of electrons inside molecules within the valence bond theory of octet bonding. It entails creating several Lewis structures that, when combined, reflect the molecule's entire electronic structure. One Lewis diagram cannot explain the bonding (lone pair, double bond, octet) elaborately. A hybrid describes a combination of possible resonance structures that represents the entire delocalization of electrons within the molecule.
Using Molecular Structure To Predict Equilibrium
Equilibrium does not always imply an equal presence of reactants and products. This signifies that the reaction reaches a point when reactant and product quantities remain constant as the rate of forward and backward reaction is the same. Molecular structures of various compounds can help in predicting equilibrium.
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![**Reaction of Benzene with Bromine to Prepare Bromobenzene**
A student reacts benzene, \( \text{C}_6\text{H}_6 \), with bromine, \( \text{Br}_2 \), to prepare bromobenzene, \( \text{C}_6\text{H}_5\text{Br} \), and hydrobromic acid (HBr).
**Chemical Reaction:**
\[ \text{C}_6\text{H}_6 + \text{Br}_2 \rightarrow \text{C}_6\text{H}_5\text{Br} + \text{HBr} \]
**Questions:**
1. What is the theoretical yield of bromobenzene in this reaction when 39.3 g of benzene reacts with 61.8 g of bromine?
- **Answer:** _______ grams
2. Which chemical is the limiting reactant?
- **Select an answer:**
3. If the actual yield of bromobenzene was 31.7 g, what was the percent yield?
- **Answer:** _______ %
**Explanation:**
This exercise involves stoichiometry and understanding the concept of limiting reactants in a chemical reaction. You will calculate the theoretical yield based on the reactants provided, determine which of the reactants limits the reaction, and then calculate the percent yield based on the actual product obtained.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F08a1092a-53fa-45f1-8cc5-326ab3991212%2F03c0e833-95eb-4582-a0e2-4e78a15cd9e7%2Fderc3a3_processed.png&w=3840&q=75)
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