1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
Dmitriy789 [7]
3 years ago
12

The expression of the theoretical yield (TY) in function of limiting reagent (LR) of a reaction is as follows: TY = ideal mole r

atio of (target product / LR) x #mol(LR) x MW(target product) The ideal mole ratio is the one provided by the equation of the reaction. If a reaction uses (4.50x10^0) g of aniline and 1.25 times as many mL of acetic anhydride as the number of grams of aniline, what is the theoreticl yiled of acetanilide (MW = 135.17 g/mol) in the reaction?
Chemistry
1 answer:
spin [16.1K]3 years ago
3 0

<u>Answer:</u> The theoretical yield of acetanilide is 6.5 grams.

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}      .....(1)

  • <u>For aniline:</u>

Given mass of aniline = 4.50\times 10^0=4.50g      (We know that:  10^0=1 )

Molar mass of aniline = 93.13 g/mol

Putting values in equation 1, we get:

\text{Moles of aniline}=\frac{4.50g}{93.13g/mol}=0.048mol

  • <u>For acetic anhydride:</u>

To calculate the mass of acetic anhydride, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Volume of acetic anhydride = (1.25\times \text{Mass of aniline})=1.25\times 4.50=5.625mL

Density of acetic anhydride = 1.08 g/mL

Putting values in above equation:

1.08g/mL=\frac{\text{Mass of acetic anhydride}}{5.625mL}\\\\\text{Mass of acetic anhydride}=(1.08g/mL\times 5.625mL)=6.08g

Given mass of acetic anhydride = 6.08 g

Molar mass of acetic anhydride = 102.1 g/mol

Putting values in equation 1, we get:

\text{Moles of acetic anhydride}=\frac{6.08g}{102.1g/mol}=0.06mol

The chemical equation for the reaction of aniline and acetic anhydride follows:

C_6H_5NH_2+CH_3COOCOCH_3\rightarrow C_6H_5NHCOCH_3+CH_3COOH

By Stoichiometry of the reaction:

1 mole of aniline reacts with 1 mole of acetic anhydride

So, 0.048 moles of aniline will react with = \frac{1}{1}\times 0.048=0.048mol of acetic anhydride

As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.

Thus, aniline is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of aniline produces 1 mole of acetanilide

So, 0.048 moles of aniline will produce = \frac{1}{1}\times 0.048=0.048mol of acetanilide

Now, calculating the theoretical yield of acetanilide by using equation 1:

Moles of acetanilide = 0.048 moles

Molar mass of acetanilide = 135.17 g/mol

Putting values in equation 1, we get:

0.048mol=\frac{\text{Mass of acetanilide}}{135.17g/mol}\\\\\text{Mass of acetanilide}=(0.048mol\times 135.17g/mol)=6.5g

Hence, the theoretical yield of acetanilide is 6.5 grams.

You might be interested in
How many
Aleksandr-060686 [28]

Answer:

A. 1.50

Explanation:

9.01 x 1023 molecules* 1 mol/ 6.022×1023 molecules= 1.49618067087 moles

Rounded would be 1.50

5 0
2 years ago
A sample of oxygen gas has a volume of 45.8 mL when its pressure is 0.492 atm. What
White raven [17]

Answer:

<h2> a. 23.6</h2>

Explanation:

P_1=0.492\:atm\\V_1 = 45.8\:ml\\V_2 = ?\\P_1 = 0.954\:atm\\\\Boyle's Law = P_1V_1 = P_2V_2\\\\Lets \:make\: V \:subject\:of\:the\:formula\\\\\frac{P_1V_1}{P_2} = \frac{P_2V_2}{P_2} \\ \\V_2 =\frac{P_1V_1}{P_2} \\V_2 = \frac{0.492\times45.8}{0.954}\\ \\V_2 = \frac{22.5336}{0.954} \\\\V_2  = 23.620\\\\V_2 = 23.6

4 0
3 years ago
Read 2 more answers
What mass of octane must be burned in order to liberate 5270 kj of heat? δhcomb = -5471 kj/mol?
katrin2010 [14]
As,
                           5471 kJ heat is given by  =  1 mole of Octane
Then,
                    5310 kJ heat will be given by  = X moles of Octane

Solving for X,
                                  X  =  (5310 kJ × 1 mol) ÷ 5471 kJ

                                  X  =  0.970 moles of Ocatne

So, 0.970 moles of Octane will liberate 5310 kJ energy. Now changing moles to mass,
As,
                                  Moles  =  mass / M.mass
Or,
                                  Mass  =  Moles × M.mass
Putting values,
                                  Mass  =  0.970 mol × 114.23 g/mol

                                  Mass  =  110.83 g of Octane
6 0
3 years ago
A student prepares a 0.47mM aqueous solution of acetic acid CH3CO2H. Calculate the fraction of acetic acid that is in the dissoc
Aliun [14]

The fraction of acetic acid that is dissociated is 0.18

Why?

The chemical equation for the dissociation of acetic acid (HAc) is the following:

HAc(aq) + H₂O(l) ⇄ H₃O⁺(aq) + Ac⁻(aq)

To find the fraction of acetic acid that is in the dissociated form (f), we apply the following equation (Ka for acetic acid is 1.76*10⁻⁵). This equation comes from solving the equation of the equilibrium constant for the dissociated fraction of HAc:

f=\frac{-Ka+\sqrt{Ka^{2} +4KaC} }{2C} = 0.18

Have a nice day!

#LearnwithBrainly

6 0
3 years ago
Strong versus weak acids what makes a strong acid strong pogil answer key
Over [174]
An acid is deemed strong if it can readily or easy "donate" a proton (H+) to the other ions in the solutions. Also, to donate or lose the proton or H+, the acid must dissociate (split into ions) in the solution. The more it can readily dissociate, the stronger the acid is.
8 0
3 years ago
Read 2 more answers
Other questions:
  • Someone who occupies a key role in the design, construction, and management of chemical operations to insure and improve the qua
    13·1 answer
  • Drag the description to the category
    11·1 answer
  • The synthesis of dipropyl ether can be accomplished using 1-propanol. What reactants and conditions are necessary for this to oc
    15·1 answer
  • Determine the value of the equilibrium constant, Kgoal, for the reaction CO2(g)⇌C(s)+O2(g), Kgoal=? by making use of the followi
    11·1 answer
  • Which best identifies why the rusting of an iron nail in the presence of water and oxygen is an oxidation-reduction reaction?
    6·1 answer
  • Example of exothermic reaction:
    7·1 answer
  • What charge will an ion of phosphorus form?
    8·2 answers
  • Answerr fasttt pleaseee lets see who can answer
    13·1 answer
  • Name the following hydrate Pb(CIO3)4 . H2O
    10·1 answer
  • Which of the following IS NOT an ionic compound?<br> A) C2H5OH<br> B) KCI<br> C) Mg3N2<br> D) MnO2
    6·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!