Question

A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr. C6H6 +...

A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr.

C6H6 + Br2--> C6H5Br + HBr

What is the theoretical yield of bromobenzene in this reaction when 0.53 moles of benzene reacts with 0.35 moles of bromine?   Incorrect moles

Which chemical is the limiting reactant?   Select an answer C6H5Br there is no limiting reactant C6H6 HBr Br2

If the actual yield of bromobenzene was 0.33 moles, what was the percent yield?   

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Benzene,C6H6(ℓ), reacts with bromine, Br2 to form bromobenzene, C6H5Br(ℓ) as described below C6H6(ℓ)    +    Br2(ℓ)   →...
Benzene,C6H6(ℓ), reacts with bromine, Br2 to form bromobenzene, C6H5Br(ℓ) as described below C6H6(ℓ)    +    Br2(ℓ)   →        C6H5Br(ℓ)       +         HBr(g) Calculate the amount of bromobenzene, C6H5Br(ℓ), in grams that can be produced from reaction of 30.0 g of C6H6 and 50.0 g Br2? Molar Mass C6H6 = 78.11 g/mol    Molar Mass Br2 = 159.8 g/mol     Molar Mass C6H5Br = 157.0 g/mol Hint: This is a limiting reactant problem.
What is the theoretical yield of bromobenzene in this reaction when 27.0g of benezene reacts with...
What is the theoretical yield of bromobenzene in this reaction when 27.0g of benezene reacts with 58.5 g of bromine? C6H6 + Br2 = C6H5Br + HBr
Part A What is the theoretical yield of bromobenzene in this reaction when 35.0 g of...
Part A What is the theoretical yield of bromobenzene in this reaction when 35.0 g of benzene reacts with 75.8 g of bromine? m = 70.3 g Part B If the actual yield of bromobenzene was 65.4 g , what was the percentage yield?
1. A student reacts 1.60 ml of 15.7M HNO3 with 0.5000g of copper metal.  Determine the limiting...
1. A student reacts 1.60 ml of 15.7M HNO3 with 0.5000g of copper metal.  Determine the limiting reactant and the amount of excess reactant (in moles) left over, assuming the reaction goes to completion. 2. A student dissolves 5.0000g CoCl2*6H2O(s) in water, reactsit with excess C2H8N2 and obtains 4.0000g of solid [Co(C2H8N2)3]Cl2 after filtering and drying the product. What is his percent yield, assuming there are no other cobalt‐containing reactants or products? 3. A student was given 15.0 ml of a...
C alcium oxide reacts with water in a combination reaction to produce calcium hydroxide: 2 2...
C alcium oxide reacts with water in a combination reaction to produce calcium hydroxide: 2 2 CaO (s) H O (l)Ca(OH) (s)  In a particular experiment, a 5.00-g sample of CaO is reacted with 125 g of water and 6.11 g of is recovered. 2 Ca(OH) a. How many moles of each reactant are present? (Show all work below) (2 pt) ______________ moles CaO ______________ moles H2O b. Which is the limiting reagent? ______________ is the limiting reagent. (Show...
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +     
1. Given the following reaction     2C2H6(l)   +      7 O2(g)   ®           4CO2(g)      +        6H2O(l) How many moles of water are produced when 4.5 moles of oxygen react?        (Hint: Use slides 5-8) 2. Given: I2     +    3 F2      ®     2 IF3 How many moles of I2 are needed to form 3 moles of IF3? How many moles of F2 are needed to form 10 moles of IF3? How many moles of I2 are needed to react with 3.5 moles of F2?        ...
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385...
Given the following experimentally determined values, answer the questions. .009070 mol Cl .00565 mol Cu .00385 mol Zn Ratio of Chloride to copper = 1.61:1 Ratio of chloride to zinc = 2.36:1 Ratio of zinc to copper = .681:1 What are your experimentally-determined formulas for (i) copper chloride, and (ii) zinc chloride? Once you have calculated the moles of each element/ion (Cu, Zn, and Cl– ), you can then determine the empirical formula of copper chloride by computing the ratio...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT