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3 years ago

What is the percent yield of LiCl if I produced 30.85g LiCl and my theoretical yield was calculated to be 35.40g LiCl?

Chemistry

1 answer:

marissa [1.9K]3 years ago

7 0

Answer:

87.15%

Explanation:

To find percent yield, we can use this simple equation

$\frac{Actual}{Theoretical} *100$

Where "Actual" is the amount in grams actually collected from the reaction, and "Theoretical" is, well, the theoretical amount that should have been produced.

They give us these values, so to find the percent yield, just plug the numbers in.

$\frac{30.85}{35.40} *100\\\\ =87.15$

So, the percent yield is 87.15%

An easy trick to remember how to do this is just to divide the smaller number by the bigger number and move the decimal back two places. If you have a percent yield greater than 100%, something is wrong in the reaction.

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The density of concentrated ammonia, which is 28.0% w/w nh3, is 0.899 g/ml. what volume of this reagent should be diluted to 1.0

vlada-n [284]

Answer: 2.4 ml

Solution :

Molar mass of $NH_3$ = 17 g/mole

Given,: 28% w/w of $NH_3$ solution means 28 g of ammonia in 100 g of solution.

Mass of solution = 100 g

Now we have to calculate the volume of solution.

$Volume=\frac{Mass}{Density}=\frac{100g}{0.899g/ml}=111.2ml$

Molarity : It is defined as the number of moles of solute present in one liter of solution.

$Molarity=\frac{n\times 1000}{V_s}$

where,

n = moles of solute $NH_3=\frac{\text {given mass}}{\text {molar mass}}=\frac{28}{17}=1.65moles$

$V_s$ = volume of solution in liter = 0.11 L

Now put all the given values in the formula of molarity, we get

$Molarity=\frac{1.65moles}{0.11L}=15mole/L$

Using molarity equation:

$M_1V_1=M_2V_2$

$15\times V_1=0.036\times 1.0\times 10^{3}$

$V_1=2.4ml$

6 0

3 years ago

Define saturated and unsaturated fats

saul85 [17]

Answer:

SATURATED: Saturated fat is a type of fat in which the fatty acid chains have all or predominantly single bonds.

UNSATURATED: Unsaturated fats are loosely packed. They tend to be liquid at room temperature.

<em>There are two main types of unsaturated fat:</em>

<u>Monounsaturated</u>

<u>Polyunsaturated</u>

8 0

3 years ago

Imagine mixing 1 tablespoon of Epsom salt with 2 cups of ammonia. How much precipitate would be produced? Describe the amount of

barxatty [35]

The amount of precipitate produced will be proportional to the amount of NH₃ reacted with water to produce NH₄OH.

<h3>What is precipitate?</h3>

Precipitates are the crystal type formation, when the solute is no more dissolving in the solvent.

Imagine mixing 1 tablespoon of Epsom salt with 2 cups of ammonia, the reaction is

2NH₃ + MgSO₄ + 2H₂O → Mg(OH)₂ + (NH₄)₂SO₄

The amount of precipitate produced will be proportional to the amount of NH₃ reacted with water to produce NH₄OH.

Learn more about precipitate.

brainly.com/question/18109776

#SPJ1

4 0

1 year ago

50 points I need help on this whole work sheet about converting moles

kozerog [31]

Answer:

Explanation:

11)

Answer:

9.08 mol

Given data:

Number of moles of P₂O₅ = ?

Number of moles of O₂ = 22.7 mol

Solution:

Chemical equation:

4P + 5O₂ → 2P₂O₅

Now we will compare the moles of P₂O₅ with O₂.

O₂ : P₂O₅

5 : 2

22.7 : 2/5×22.7 = 9.08

12)

Answer:

7 mol

Given data:

Number of moles of P₂O₅ = ?

Number of moles of P = 14 mol

Solution:

Chemical equation:

4P + 5O₂ → 2P₂O₅

Now we will compare the moles of P₂O₅ with P.

P : P₂O₅

4 : 2

14 : 2/4×14 = 7

13)

Answer:

76.25 mol

Given data:

Number of moles of P = 61 mol

Number of moles of O₂ react = ?

Solution:

Chemical equation:

4P + 5O₂ → 2P₂O₅

Now we will compare the moles of P with O₂.

P : O₂

4 : 5

61 : 5/4×61 = 76.25

14)

Answer:

1.25 mol

Given data:

Number of moles of P₂O₅ = 0.5 mol

Number of moles of O₂ needed = ?

Solution:

Chemical equation:

4P + 5O₂ → 2P₂O₅

Now we will compare the moles of P₂O₅ with O₂.

P₂O₅ : O₂

2 : 5

0.5 : 5/2×0.5 = 1.25

15)

Answer:

20 mol

Given data:

Number of moles of P₂O₅ = 8 mol

Number of moles of O₂ needed = ?

Solution:

Chemical equation:

4P + 5O₂ → 2P₂O₅

Now we will compare the moles of P₂O₅ with O₂.

P₂O₅ : O₂

2 : 5

8 : 5/2×8 = 20

16)

Answer:

12 mol

Given data:

Number of moles of silver made = ?

Number of moles of Ag₂O = 6 mol

Solution:

Chemical equation:

2Ag₂O → 4Ag + O₂

Now we will compare the moles of Ag with Ag₂O .

Ag₂O : Ag

2 : 4

6 : 4/2×6 = 12

17)

Answer:

25 mol

Given data:

Number of moles of silver made = ?

Number of moles of O₂ produced = 6.25 mol

Solution:

Chemical equation:

2Ag₂O → 4Ag + O₂

Now we will compare the moles of Ag with O₂ .

O₂ : Ag

1 : 4

6.25 : 4×6.25 = 25

18)

Answer:

9.8 mol

Given data:

Number of moles of silver made = ?

Number of moles of O₂ produced = 2.45 mol

Solution:

Chemical equation:

2Ag₂O → 4Ag + O₂

Now we will compare the moles of Ag with O₂ .

O₂ : Ag

1 : 4

2.45 : 4×2.45 = 9.8

19)

Answer:

4.4 mol

Given data:

Number of moles of silver oxide required = ?

Number of moles of O₂ produced = 2.2 mol

Solution:

Chemical equation:

2Ag₂O → 4Ag + O₂

Now we will compare the moles Ag₂O of with O₂ .

O₂ : Ag₂O

1 : 2

2.2 : 2×2.2 = 4.4

20)

Answer:

1.5 mol

Given data:

Number of moles of silver oxide required = ?

Number of moles of O₂ produced = 0.75 mol

Solution:

Chemical equation:

2Ag₂O → 4Ag + O₂

Now we will compare the moles Ag₂O of with O₂ .

O₂ : Ag₂O

1 : 2

0.75 : 2×0.75 = 1.5

8 0

3 years ago

Sucrose is very soluble in water. at 25◦c, 211.4 grams of sucrose will dissolve in 100 g of water. given that the density of the

stiv31 [10]

Molarity of solution is mathematically expressed as,
M = $\frac{x\text{weight of solute(g)}}{\text{Molecular weight X Volume of solution(l)}}$

We know that volume = mass/density
Given: mass of solution = 100 g, Density = 1.34 g/ml
∴ volume = 100/1.34 = 88.49 ml = 0.08849 l

Also, we know that molecular weight of sucrose = 342.3 g/mol
∴M = $\frac{x\text{211.4}}{\text{342.3 X 0.08849}}$
= 6.979 M

Thus, molarity of solution is 6.979 M

8 0

3 years ago