Please i needed but Good

It is desired to produce 2.25 grams of dichloromethane (CH2Cl2) by the following reaction. If the percent yield of dichlorometha

Allushta [10]

Answer:- 3.12 g carbon tetrachloride are needed.

Solution:- The balanced equation is:

$CH_4+CCl_4\rightarrow 2CH_2Cl_2$

From given actual yield and percent yield we will calculate the theoretical yield that would be further used to calculate the grams of carbon tetrachloride.

percent yield formula is:

percent yield = $(\frac{actual}{theoretical})100$

$65.5=(\frac{2.25}{theoretical})100$

$theoretical=(\frac{2.25(100)}{65.5})$

theoretical = 3.44 g

From balanced equation, there is 2:1 mol ratio between dichloethane and carbon tetrachloride.

Molar mass of dichloroethane is 84.93 gram per mol and molar mass of carbon tetrachloride is 153.82 gram per mol.

$3.44gCH_2Cl_2(\frac{1molCH_2Cl_2}{84.93gCH_2Cl_2})(\frac{1molCCl_4}{2molCH_2Cl_2})(\frac{153.82gCCl_4}{1molCCl_4})$

= $3.12gCCl_4$

So, 3.12 grams of carbon tetrachloride are needed to be reacted.

8 0

2 years ago

For a reaction 2A + B 2C, with the rate equation: Rate = k[A]2[B]

In-s [12.5K]

For reaction

2 A + B ------------> 2 C

Rate = K [ A ]² [ B ]

<span> the order with respect to A is 2 and the order overall is 3.
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hope this helps!

3 0

2 years ago

Determine the freezing point and boiling point of a solution that has 68.4 g of sucrose

Ymorist [56]

Answer:

Freezing T° of solution = - 3.72°C

Boiling T° of solution = 101.02°C

Explanation:

To solve this we apply colligative properties. Firstly, freezing point depression:

ΔT = Kf . m . i

ΔT = Freezing T° of pure solvent - Freezing T° of solution

Kf = Cryoscopic constant, for water is 1.86 °C/m

m = molality (moles of solute in 1kg of solvent)

i = Ions dissolved in solution

Our solute is sucrose, an organic compound so no ions are defined. i = 1.

Let's determine the moles: 68.4 g . 1mol/ 342g = 0.2 moles

molality = 0.2 mol / 0.1kg of water = 2 m

We replace data: ΔT = 1.86°C/m . 2m . 1

Freezing T° of solution = - 3.72°C

Now, we apply elevation of boiling point: ΔT = Kb . m . i

ΔT = Boiling T° of solution - Boiling T° of pure solvent

Kf = Ebulloscopic constant, for water is 0.512 °C/m

We replace:

Boiling T° of solution - Boiling T° of pure solvent = 0.512 °C/m . 2 . 1

Boiling T° of solution = 0.512 °C/m . 2 . 1 + 100°C → 101.02°C

6 0

2 years ago

What reaction is zinc(s) + water(l) →

Marat540 [252]

Answer:

Zn+H2O ------ ZnO + H2 is the correct answer

8 0

2 years ago

Read 2 more answers

A gas in a sealed container had its volume increased from 12.1 liters to 21.1 liters.

ArbitrLikvidat [17]

Answer:

The answer to your question is P2 = 170.9 torr

Explanation:

Data

Volume 1 = 12.1 l Volume 2 = 21.1 l

Temperature 1 = 241 °K Temperature 2 = 298°K

Pressure 1 = 546 torr Pressure 2 = ?

Process

To solve this problem use the combined gas law.

P1V1/T1 = P2V2/T2

-Solve for P2

P2 = T1V1T2 / T1V2

-Substitution

P2 = (241 x 12.1 x 298) / (241 x 21.1)

-Simplification

P2 = 868997.8 / 5085.1

-Result

P2 = 170.9 torr

8 0

3 years ago